Name: Date: Hour: Chemistry Final Exam Review: herberholz
|
|
- Aubrey Parks
- 6 years ago
- Views:
Transcription
1 Name: Date: Hour: Chemistry Final Exam Review: herberholz Many concepts and skills from first semester will be needed to be successful on the final exam. In addition to this semester s material you should also review key 1 st semester topics. Common topics from 1 st semester that you should review include: naming compounds and writing formulas, dimensional analysis, and significant figure rules. This review is worth 5% extra credit to your final exam. It is due the day you are scheduled to take your final. Your work must be hand written and it must be your own work. Copying answers from another student will not help you to be successful on this exam. Be sure to answer every question. For calculation questions, you must show your work to receive credit. Chapter 11: 1) What are the different types of reactions? 2) How do you determine if a precipitate has formed in a reaction? 3) What is a catalyst? 4) Rewrite the word equation as balanced chemical equations. a. hydrogen + sulfur hydrogen sulfide b. iron(iii) chloride + calcium hydroxide iron(iii) hydroxide + calcium chloride 5) Balance the following equations. a. SO 2 + O 2 SO 3 b. Fe 2O 3 + H 2 Fe + H 2O c. P + O 2 P 4O 10 d. Al + N 2 AlN 6) Complete and balance this equation for a combination reaction. Be + O 2 7) Complete and balance this decomposition reaction. HI 8) Complete the equations for these single replacement reactions in aqueous solution. Balance each equation. a. Fe(s) + Pb(NO 3) 2(aq) b. Cl 2(aq) + NaI(aq) c. Ca(s) + H 2O(l) 9) Write the products of these double replacement reactions. Then balance each equation. a. NaOH(aq) + Fe(NO 3) 3(aq) Note: Iron(III) Hydroxide is a precipitate. 1
2 b. Ba(NO 3) 2(aq) + H 3PO 4(aq) Note: Barium phosphate is a precipitate. 10) What are the five types of chemical reactions? 11) Classify each reaction and balance the equation. a. C 3H 6 + O 2 CO 2 + H 2O b. Al(OH) 3 Al 2O 3 + H 2O c. Li + O 2 Li 2O d. Zn + AgNO 3 Ag + Zn(NO 3) 2 12) Write the balanced net ionic equation for each reaction and identify the spectator ions in each reaction. a. Pb(NO 3) 2(aq) + H 2SO 4(aq) PbSO 4(s) + HNO 3(aq) b. Pb(C 2H 3O 2) 2(aq) + HCl(aq) PbCl 2(s) + HC 2H 3O 2(aq) c. Na 3PO 4(aq) + FeCl 3(aq) NaCl(aq) + FePO 4(s) d. (NH 4) 2S(aq) + Co(NO 3) 2(aq) CoS(s) + NH 4NO 3(aq) 13) Identify the reactants and products in each chemical reaction. a. Hydrogen gas and sodium hydroxide are formed when sodium is dropped into water. b. In photosynthesis, carbon dioxide and water reacted to form oxygen gas and glucose. 14) What is the purpose of a catalyst? Chapter 12: 1) What is the difference between limiting and excess reagent? 2) Interpret the equation for the formation of water from its elements in terms of number of molecules and moles, and volumes of gases at STP. 2H 2(g) + O 2(g) 2H 2O(g) 2
3 3) Chemical reactions can be described in terms of what quantities? 4) What quantities are always conserved in chemical reactions? 5) Interpret the given equation in terms of relative numbers of representative particles, numbers of moles, and masses of reactants and products. 2K(s) + 2H 2O(l) 2KOH(aq) + H 2(g) 6) According to the following equation: 4Al(s) + 3O 2(g) 2Al 2O 3(s). a. How many moles of oxygen are required to react completely with 14.8 mol Al? b. How many moles of Al 2O 3 are formed when 0.78 mol O 2 reacts with aluminum? 7) Acetylene gas (C 2H 2) is produced by adding water to calcium carbide (CaC 2). CaC 2(s) + 2H 2O(l) C 2H 2(g) + Ca(OH) 2(aq) a. How many grams of acetylene are produced by adding water to 5.00 g CaC 2? b. Determine how many moles of CaC2 are needed to react with 49.0 g H 2O. 8) How many molecules of oxygen are produced by the decomposition of 6.54 g of potassium chlorate (KClO 3)? KClO 3(s) 2KCl(s) + 3O 2(g) 9) The equation for the combustion of carbon monoxide is: 2CO(g) + O 2(g) 2CO 2(g). How many liters of oxygen are required to burn 3.86 L of carbon monoxide? 10) Consider the following equation: CS 2(l) + 3O 2(g) CO 2(g) + 2SO 2(g). Calculate the volume of sulfur dioxide produced when 27.9 ml O 2 reacts with carbon disulfide. 11) The equation for the complete combustion of ethane (C 2H 4) is: C 2H 4(g) + 3O 2(g) 2CO 2(g) + 2H 2O(g). If 27.0 mol C 2H 4 is reacted with 6.30 mol O 2, identify the limiting reagent. 3
4 12) The following equation shows the incomplete combustion of ethane: C 2H 4(g) + 3O 2(g) 2CO(g) + 2H 2O(g). If 2.70 mol C 2H 4 is reated with 6.30 mol O 2. a. Identify the limiting reagent. b. Calculate the moles of water produced. 13) When 84.8 g of iron (III) oxide reacts with an excess of carbon monoxide, iron is produced. Fe 2O 3(s) + 3CO(g) 2Fe(s) + 3CO 2(g) What is the theoretical yield of iron? 14) If 50.0 g of silicon dioxide is heated with an excess of carbon, 27.9 g of silicon carbide is produced. SiO 2(s) + 3C(s) SiC(s) + 2CO(g) What is the percent yield of this reaction? 15) In a chemical reaction, how does an insufficient quantity of a reactant affect the amount of product formed? 16) The reaction of fluorine with ammonia produces dinitrogen tetrafluoride and hydrogen fluoride. 5F 2(g) + 2NH 3(g) N 2F 4(g) + 6HF(g) a. If you have 66.6 g NH 3, how many grams of F 2 are required for complete reaction? b. How many grams of NH 3 are required to produce 4.65 g HF c. How many grams of N 2F 4 can be produced from 225 g F 2? 17) Lithium nitride reacts with water to form ammonia and aqueous lithium hydroxide. Li 3N(s) + 3H 2O(l) NH 3(g) + 3LiOH(aq) a. What mass of water is needed to react with 32.9 g Li 3N? b. When the above reaction takes place, how many molecules of NH 3 are produced? c. Calculate the number of grams of Li 3N that must be added to an excess of water to produce 15.0 L NH 3 (at STP). 4
5 18) What is the significance of the limiting reagent in a reaction? What happens to the amount of any reagent that is present in an excess? 19) In a reaction chamber, 3.0 mol of aluminum is mixed with 5.3 mol Cl2 and reacts. The reaction is described by the following balanced chemical equation: 2Al + 3Cl 2 2AlCl 3. a. Identify the limiting reagent for the reaction. b. Calculate the number of moles of product formed. c. Calculate the number of moles of excess reagent remaining after the reaction. Chapter 13: 1. What pressure (in kilopascals) does a gas exert when at 678 mm of Hg? 2. What pressure (in atmospheres) does a gas exert when at 678 mm of Hg? 3. Describe the basic assumption of the kinetic theory of gases. 4. In terms of kinetic energy, explain how a molecule in a liquid evaporates. 5. With regards to vapor pressure, what must occur for a liquid to boil? 6. What two phases are in equilibrium at a substance s melting point? 7. What two phases are in equilibrium at a substance s boiling point? 8. How do the melting points of ionic solids and molecular solids differ? Explain your answer. 9. Describe what is happening at the molecular level when dynamic equilibrium occurs in a closed container. (Hint: what are the molecules doing while at dynamic equilibrium?) 10. Name one physical property that you could use to distinguish between molecular and ionic solids. 11. What does the term STP mean? 12. What is the effect of temperature on vapor pressure? 5
6 13. Explain the term Normal Boiling Point and what must the air pressure be at Normal Boiling Point. Chapter 14: 1. In a given container, name two ways in which you can increase and decrease pressure. 2. Distinguish between Boyle s law and Charles s Law 3. What is the combined gas law? 4. How is the ideal gas law used? 5. What is the law of partial pressures? 6. List 3 factors that can affect gas pressure. 7. If the temperature is constant, what change in volume would cause the pressure of an enclosed gas to be reduced to ¼ of its original value? Which gas law are you using in this problem? 8. The pressure on 2.50 L of N 2O changes from 105 kpa to 40.5 kpa. If the temperature remains constant, what will the new volume be? Which gas law are you using in this problem? 9. If a sample of gas occupies 6.80 L at 325 C, what will its volume be at 25 C if the pressure remains constant? Which gas law are you using in this problem? 10. The pressure in a car tire is 198 kpa at 27 C. After a long drive, the pressure is 225 kpa. In a rigid container where volume remains constant, what is the temperature of the air in the tire? Which gas law are you using in this problem? 11. A gas at 155 kpa and 25 C has an initial volume of 1.00 L. The pressure of the gas increases to 605 kpa as the temperature is raised to 125 C. What is the new volume? Which gas law are you using in this problem? 6
7 12. How are pressure and volume of a gas related at constant temperature? Explain using the terms Direct or Inverse relationship. 13. How are pressure and temperature of a gas related at constant volume? Explain using the terms Direct or Inverse relationship. 14. How are temperature and volume of a gas related at constant pressure? Explain using the terms Direct or Inverse relationship. 15. Write the formulas for Boyle s Law, Charles Law, and Gay Lussac s Law. 16. When the temperature of a rigid hollow sphere containing 685 L of helium gas is held at 621 K, the pressure of the gas is 1.89 x 10 3 kpa. How many moles of helium does the sphere contain? Which gas law are you using in this problem? 17. A container has a volume of 2.20 L. How many grams of nitrogen gas will the container hold at a pressure of 102 kpa and a temperature of 37 C? 18. What pressure is exerted by moles of a gas at 25 C if the gas is a L container? 19. In your own words, state Dalton s Law of partial pressures. 20. How is the partial pressure of a gas in a mixture calculated? 21. Determine the total pressure of a gas mixture that contains oxygen, nitrogen, and helium if the partial pressures are P oxygen= 20.0 kpa, P nitrogen=46.7 kpa, and P helium=26.7 kpa. 22. Explain why heating a contained gas that is held at a constant volume increases its pressure. Chapter 15: 1. What causes the high surface tension and low vapor pressure of water? 7
8 2. What effect does a surfactant have on the surface tension of water? 3. What is the percent by mass of water in CuSO 4 5H 2O 4. In the formation of a solution, how does the solvent differ from the solute? 5. Why are all ionic compounds electrolytes? 6. Which of the following substances dissolve to a significant extent in water? Explain your answer in terms of polarity. a. CH 4 b. KCl c. He d. MgSO 4 e. Sucrose f. NaHCO 3 7. How does a suspension differ from a solution? 8. What distinguishes a colloid from a suspension and a solution? 9. Why is water an excellent solvent for most ionic and polar covalent compounds but not for a nonpolar compound? 10. What is the main distinction between an aqueous solution of a strong electrolyte and an aqueous solution of a weak electrolyte? 11. Write formulas for these hydrates: a. Sodium sulfate hexahydrate b. Calcium chloride trihydrate c. Barium hydroxide octahydrate 12. Name each hydrate: 8
9 a. SnCl 4 5H 2O b. FeSO 4 7H 2O c. BaBr 2 4H 2O d. FePO 4 4H 2O 13. Arrange colloids, suspensions, and solutions in order of increasing particle size. 14. What is hydrogen bonding and how does it work? 15. What is surface tension? 16. What is a surfactant? 17. What is the difference between a solute, a solvent, a solution, and a suspension? 18. What is the Tyndall effect? 19. What is Brownian motion? Chapter 16: 1. The solubility of a gas in water is 0.16 g/l at 104 kpa. What is the solubility when the pressure of the gas is increased to 288 kpa? Assume constant temperature. 2. What factor determines whether a substance will dissolve in a specific solvent? 3. What 3 factors determine the rate at which a solute dissolves? 4. What units are usually used to express the solubility of a solute? 5. A solution has a volume of 2.0 L and contains 36.0 g of glucose (C 6H 12O 6). If the molar mass of glucose is 180 g/mol, what is the molarity of the solution? 9
10 6. How many moles of ammonium nitrate are in 335 ml of M NH 4NO 3? 7. How many milliliters of a solution of 4.00 M KI are needed to prepare ml of M KI? 8. If 10 ml of propanone is diluted with water to a total solution volume of 200 ml, what is the percent by volume of the propanone in the solution? 9. What are two ways of expressing the concentration of a solution as a percent? 10. How many grams of K 2SO 4 would you need to prepare 1500 ml of 5% K 2SO 4 (m/v) solution? 11. An equal number of moles of KI and MgI 2 are dissolved in equal volumes of water. Which solution has the higher: a. Boiling point? b. Vapor pressure? c. Freezing point? 12. Define the following terms: solubility, saturated solution, and unsaturated solution. 13. Knowing the molarity of a solution is more meaningful than knowing whether a solution is dilute or concentrated. Explain. 14. What are colligative properties? Identify 3 colligative properties and explain why each occurs. 15. Compare the terms molarity and dilution. Chapter 17: 1. When solid barium hydroxide octahydrate (Ba(OH) 2 8H 2O) is mixed in a beaker with solid ammonium thiocyanate (NH4SCN) a reaction occurs. The beaker becomes very cold. Is this reaction exothermic or endothermic? 10
11 2. When 435J of heat is added to 3.4g of olive oil at 21 C the temperature will increase to 85 C. What is the specific heat of olive oil? 3. How much heat is required to raise the temperature of 250.0g of mercury 52 C? 4. How do endothermic processes differ from exothermic processes? 5. On what factors does the heat capacity of an object depend? 6. When 50.0mL of water containing 0.50 mol HCl at 22.5 C is mixed with 50.0mL of water containing 0.50 mol NaOH in a calorimeter, the temperature of the solution increases to 26.0 C. How much heat (in kj) was released by this reaction? 7. When carbon disulfide is formed from its elements, heat is absorbed. Calculate the amount of heat (in kj) absorbed when 5.66g of carbon disulfide is formed. C(s) + 2S2(s) CS 2(l) H= 89.3kJ 8. How are enthalpy changes treated in a chemical reaction? 9. How many kilojoules of heat are required to melt a 10.0g popsicle at 0 C? Assume the popsicle has the same molar mass and heat of fusion as water. 10. How much heat is absorbed when 63.7g H20(l) at 100 C at 101.3kPa is converted to steam at 100 C? Express your answer in kj. 11. How much heat in (kj) is released when mol of NaOH(s) is dissolved in water? 12. How many moles of NH4NO3(s) must be dissolved in water so that 88.0kJ of heat is absorbed from the water? 13. Define potential energy in terms of chemistry. 14. Why do you think it is important to define system and surroundings? 15. Describe the sign convention that is used thermochemical calculations. 16. What is the function of a calorimeter? 11
12 17. What information is given in a thermochemical equation? 18. What is the difference between specific heat capacity and heat capacity? 19. What is the difference between a calorie and a joule? 20. What is the difference between endothermic and exothermic? Chapter 18: 1. How is the rate of a chemical reaction expressed? 2. What are four factors that affect the rate of a chemical reaction? 3. Does every collision between reacting particles lead to products? Explain. 4. How is the equilibrium position of this reaction affected by the following changes? C(s) + H20(g) + heat CO(g) + H2(g) a. Lowering the temp b. Increasing the pressure c. Removing hydrogen d. Adding water vapor 5. The reversible reaction N2(g) + 3H2(g) 2NH3(g) produces ammonia, which is a fertilizer. At equilibrium, a 1-L flask contains 0.15mol H2, 0.25mol N2, and 0.10mol NH3. Calculate Keq for the reaction. 6. For the same mixture, under the same conditions described in problem 7, calculate Keq for 2NH3(g) N2(g) + 3H2(g). How is the Keq for a forward reaction related to the Keq for a reverse reaction? 7. At 750 the following reaction reaches equilibrium in a 1-L flask. H2(g) + CO2 H20(g) + CO(g) Analysis of the equilibrium mixture gives the following results: H2 = 0.053mol, CO2 = 0.053mol, H2O = 0.047mol, and CO = 0.047mol. Calculate the Keq for the reaction. 8. How do the amounts of reactants and products change after a reaction has reached chemical equilibrium? 9. What are the three stresses that can upset the equilibrium of a chemical reaction? 12
13 10. Using the following equilibrium constants for several reactions, determine in which reactions the products are favored? Why? a. K eq = b. K eq = c. K eq = What are two characteristics of spontaneous reactions? 12. What two factors determine the spontaneity of a reaction? 13. How is the rate of a reaction influenced by a catalyst? How do catalyst make this possible? 14. What is LeChatelier s principle? Use it to explain why carbonated drinks go flat when their containers are left open. 15. The products in a spontaneous process are more ordered that the reactants. Is the entropy change favorable or unfavorable? 16. Predict the direction of the entropy change in each reaction a. CaCO3(s) CaO(s) + CO2(g) b. NH3(g) + HCl(g) NH4Cl(s) 17. What is the difference between spontaneous and nonspontaneous reactions? 18. What is entropy? 19. Why do reactions a equilibrium tend to shift back and forth when pressure or other factors change? 20. What is the formula to determine the equilibrium constant for a reaction? Chapter Identify the following acids as monoprotic, diprotic, or triprotic. Explain your reasoning. a. H 2CO 3 b. H 3PO 4 c. HCl d. H 2SO 4 2. Classify each solution as acidic, basic, or neutral. a. [H + ] = 6.0 x M 13
14 b. [OH - ] = 3.0 x 10-2 M c. [H + ] = 2.0 x 10-7 M d. [OH - ] = 1.0 x 10-7 M 3. Find the ph of each solution. a. [H + ] = 1 x 10-4 M b. [H + ] = M 4. Calculate the [H + ] for each solution. a. ph = 5.00 b. ph = Calculate the ph of each solution. a. [OH - ] = 4.3 x 10-5 M b. [OH - ] = 4.5 x M 6. What is the relationship between [H + ] and [OH - ] in an aqueous solution? 7. What are the hydroxide-ion concentrations for solutions with the following ph values? a b c How many moles of potassium hydroxide are needed to completely neutralize 1.56 mol of phosphoric acid? 9. How many moles of sodium hydroxide are required to neutralize 0.20 mol of nitric acid? 10. What is the molarity of H 3PO 4 if 15.0 ml is completely neutralized by 38.5 ml of M NaOH? 11. What are the products of a reaction between an acid and a base? 12. Write complete balanced equations for the following acid-base reactions. a. H 2SO 4(aq) + KOH (aq) b. H 3PO 4(aq) + Ca(OH) 2(aq) 14
15 c. HNO 3(aq) + Mg(OH) 2(aq) 13. Classify each compound as an Arrhenius acid or an Arrhenius base. a. Ca(OH) 2+ d. C 2H 5COOH b. HNO 3 e. HBr c. KOH f. H 2SO Label the conjugate acid-base pairs in each equation below a. HNO 3 + H 2O H 3O + + NO 3 - b. CH 3COOH + H 2O H 3O + + CH 3COO - c. NH 3 + H 2O NH OH - d. H 2O + CH 3COO - CH 3COOH + OH What is the molarity of sodium hydroxide if 20.0 ml of the solution is neutralized by each of the following 1.00 M solutions? a ml of HCl b ml of H 3PO What is an amphoteric substance? 17. Using the ph scale, what are acids, bases, and neutral numbers? 18. What is an Arrhenius acid and base? 19. What is a Bronsted-Lowry acid and base? 20. What is a conjugate acid and base? 21. What is a Lewis acid and base? 22. What is the difference between hydrogen ion concentration and hydroxide ion concentration? 15
16 23. How do you determine ph using the hydrogen ion concentration of a solution? 24. What is a titration? Chapter Determine what is oxidized and what is reduced in each reaction. Identify the oxidizing agent and reducing agent in each case. a. 2Na (s) + S (s) Na 2S (s) b. 4Al (s) + 3O 2(g) 2Al 2O 3(s) 2. Identify these processes as either oxidation or reduction. a. 2I - I 2 + 2e - b. Zn e - Zn 3. Define oxidation and reduction in terms of the gain or loss of electrons. 4. Use electron transfer or electron shift to identify what is oxidized and what is reduced in each reaction. Use the electronegativity values in Table 6.2 in Chapter 6, for molecular compounds. a. 2Na (s) + Br 2(l) 2NaBr (s) b. H 2(g) + Cl 2(g) 2HCl (g) c. 2Li (s) + F 2(g) 2LiF (s) d. S (s) + Cl 2(g) SCl 2(g) e. N 2(g) + 2O 2(g) 2NO 2(g) f. Mg (s) + Cu(NO 3) 2(aq) Mg(NO 3) 2(aq) + Cu (s) 5. Identify the reducing agent and the oxidizing agent for each problem in #4. 6. Determine the oxidation number of chlorine in each of the following substances. a. KClO 3 c. Ca(ClO 4) 2 b. Cl 2 d. Cl 2O 7. Identify which atoms are oxidized and which are reduced in each reaction. a. 2H 2(g) + O 2(g) 2H 2O (l) b. 2KNO 3(s) 2KNO 2(g) + O 2(g) 16
17 8. How is a change in oxidation number related to the process of oxidation and reduction? 9. Identify which of the following are oxidation-reduction reactions. If a reaction is a redox reaction, name the element oxidized and the element reduced. a. Mg (s) + Br 2(l) MgBr 2(s) b. H 2CO 3(aq) H 2O (l) + CO 2(g) 10. Balance each redox equation using oxidation-number change method. a. KClO 3(s) KCl (s) + O 2(g) b. HNO 2(aq) + HI (aq) NO (g) + I 2(s) + H 2O (l) 11. Balance each redox equation using the oxidation-number change method. a. Bi 2S 3(s) + HNO 3(aq) Bi(NO 3) 3(aq) + NO (g) + S (s) + H 2O (l) b. SbCl 5(aq) + KI (aq) SbCl 3(aq) + KCl (aq) + I 2(s) 12. Which of these statements is false? a. The oxidation number of an uncombined element is zero. b. The sum of the oxidation numbers of the atoms in a polyatomic ion must equal the charge of the ion. c. Every element has a single oxidation number. d. The oxidation number of oxygen in a compound or polyatomic ion is almost always Assign oxidation numbers to the atoms in the following ions: a. Ca +2 b. Al 2S 3 c. Na 2CrO 4 d. V 2O 5 e. MnO What is the difference between a redox reaction and a non-redox reaction? Chapter List the symbol for an alpha, beta and gamma particle. Which of the three has no mass or no charge? K e Li He The half-life of radon-222 is 3.8 days. How much of the g sample is left after 15.2 days? 17
2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?
PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationC. Perform the following calculations and Round into correct scientific notation.
Name Hour Honors Chemistry Final Exam Review 2018 - HERBERHOLZ *Due on the day of the exam! No photocopying or copying other classmate s review. Must be handwritten and show work for calculations. Chapter
More informationIons in Aqueous Solutions and Colligative Properties
CHAPTER 13 REVIEW Ions in Aqueous Solutions and Colligative Properties SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Use the guidelines in Table 1 on page 437 of the text
More informationCHEMISTRY CP Name: Period:
CHEMISTRY CP Name: Period: CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the second semester. Questions are organized by chapter/concept to help
More information3. Which of the following compounds is soluble? The solubility rules are listed on page 8.
1. Classify the following reaction. Sb 2 O 3 + 3 Fe 2 Sb + 3 FeO a) Combination reaction b) Decomposition reaction c) Neutralization reaction d) Single-replacement reaction e) Double-replacement reaction
More informationChemistry Final Exam Sample Items
Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More informationName: Period: CHEMISTRY I HONORS SEMESTER 2 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 2 EXAM REVIEW Unit 9: Stoichiometry How does the amount of each reactant present at the start of a chemical reaction determine how much product forms? How are
More information2nd Semester Exam Review. C. K eq = [N 2][H 2 ]
Name: ate: 1. Which pair of formulas represents the empirical formula and the molecular formula of a compound?. H 2 O, 4 H 6 O 4. HO, 6 H 12 O 6 8. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g)
More informationChemistry Exam Review
Chemistry Exam Review This exam review was compiled using the NC Essential Standards. You need to answer each question. You will receive multiple grades for your work. If you study everything on the exam
More informationCHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3
CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationHONORS CHEMISTRY FINAL EXAM REVIEW
HONORS CHEMISTRY FINAL EXAM REVIEW STRATEGY: Start by reading through your notes to refresh your memory on these topics. Then, use this review sheet as a starting point to identify the areas on which you
More information2) Isotopes are atoms of the same element, which have the same number of but a different number.
AP Chemistry Semester 1 Exam Review Alternate Atomic Structure 1) Fill in the table: Name Per Isotope Symbol Atomic Mass Mass # Atomic # # of protons # of neutrons # of electrons Hydrogen-1 16 16 18 35.45
More informationWater & Solutions Chapter 17 & 18 Assignment & Problem Set
Water & Solutions Chapter 17 & 18 Assignment & Problem Set Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Water & Solutions 2 Vocabulary (know
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More information2. Identify each of the following samples of matter as heterogeneous or homogeneous.
EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36
More informationName: Period: CHEMISTRY I HONORS SEMESTER 2 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 2 EXAM REVIEW Unit 9: Stoichiometry How does the amount of each reactant present at the start of a chemical reaction determine how much product forms? How are
More informationCHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More information5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?
1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole
More informationChapter 11 Thermochemistry Heat and Chemical Change
Chemistry/ PEP Name: Date: Chapter 11 Thermochemistry Heat and Chemical Change Chapter 11:1 35, 57, 60, 61, 71 Section 11.1 The Flow of Energy - Heat 1. When 435 of heat is added to 3.4 g of olive oil
More informationName Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS
SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemistry 11 Notes on Chemical Reactions Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred:
More informationSpring Semester Final Exam Study Guide
Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous
More informationRegents review Physical properties of matter
2011-2012 1. Which statement describes a chemical property of oxygen? A) Oxygen has a melting point of 55 K. B) Oxygen can combine with a metal to produce a compound. C) Oxygen gas is slightly soluble
More informationactual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information
12 Study Guide 12 Study Guide Study Tip Prioritize Schedule your time realistically. Stick to your deadlines. If your class subscribes to the Interactive Textbook with ChemASAP, your students can go online
More informationStudy Guide: Stoichiometry
Name: Study Guide: Stoichiometry Period: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE
More informationChemistry I 2nd Semester Exam Study Guide
Chemistry I 2nd Semester Exam Study Guide Study the following topics and be able to apply these concepts to answer related questions to best prepare for the Chemistry exam. You should be able to: 1. Identify
More informationAccelerated Chemistry Semester 2 Review Sheet
Accelerated Chemistry Semester 2 Review Sheet The semester test will be given in two parts. The first part is a performance assessment and will be given the day before the semester test. This will include
More informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More informationName: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationFINAL EXAM REVIEW QUESTIONS
FINAL EXAM REVIEW QUESTIONS Matter and Chemical Bonding 1) Classify each of the following as either a element, compound, a solution or a heterogeneous mixture: a) vinegar b) mercury c) brass d) potassium
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationSemester 2 Honors Chemistry Final Review
Semester 2 Honors Chemistry Final Review Name: Chapter 8 - Chemical Reactions I can balance chemical equation using the law of conservation of mass. 1. Which coefficients correctly balance the formula
More informationChemistry Spring 2018 Final Exam Review
Name Date Period Chemistry Spring 2018 Final Exam Review TURN THIS COMPLETED REVIEW IN TO YOUR TEACHER BY DAY OF YOUR FINAL FOR A 5 point FINAL EXAM BONUS Unit #7 Moles 1. What is a mole? 2. What is molar
More information(B) K2O potassium dioxide
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More informationUnit 5 Chemical Reactions Notes. Introduction: Chemical substances have physical and chemical properties
Unit 5 Chemical Reactions Notes Introduction: Chemical substances have physical and chemical properties Physical Properties 2 Types of Physical Properties Extensive Physical Properties Intensive Physical
More information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationHonors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
More informationName Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C?
Solubility Curve Practice Problems Directions: Use the graph to answer the questions below. Assume you will be using 100g of water unless otherwise stated. 1. How many grams of potassium chloride (KCl)
More informationCHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:
CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS
More information7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions
General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationStoichiometry SUPPLEMENTAL PROBLEMS CHAPTER 12. 3Si(s) 2N 2 N 4. (g) 0 Si 3. (s) PO 4. the reaction. Cr(s) H 3. (aq) 0.
CHAPTER 12 Stoichiometry 1. Silicon nitride is used in the manufacturing of high-temperature thermal insulation for heat engines and turbines. It is produced by the following 3Si(s) 2N 2 (g) 0 Si 3 N 4
More informationName Date Class CHEMICAL REACTIONS. SECTION 11.1 DESCRIBING CHEMICAL REACTIONS (pages )
Name Date Class 11 CHEMICAL REACTIONS SECTION 11.1 DESCRIBING CHEMICAL REACTIONS (pages 321 329) This section explains how to write equations describing chemical reactions using appropriate symbols. It
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationFinal Exam Review-Honors Name Period
Final Exam Review-Honors Name Period This is not a fully comprehensive review packet. This packet is especially lacking practice of explanation type questions!!! You should study all previous review sheets
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
More informationSpring Final Exam Review
Directions: Complete all of the following questions. Turn this in on the day of your final and you can earn up to 10 bonus points on your final. You must number and answer every questions on a separate
More information1.1 Introduction to the Particulate Nature of Matter and Chemical Change MATTER. Homogeneous (SOLUTIONS)
TOPIC 1: STOICHIOMETRIC RELATIONS 1.1 Introduction to the Particulate Nature of Matter and Chemical Change MATTER Mass Volume Particles Particles in constant motion MATTER Pure Matters Mixtures ELEMENTS
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
More informationAnswer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10
More information4) Convert: a) 10 m = km b) 500 g = mg c) 250 ml = L
Data Analysis 1) Define: a) Accuracy b) Precision 2) The actual density of water is 1.00 g/ml Fred Wilma Barney Trial 1 1.12 g/ml 0.88 g/ml 1.00 g/ml Trial 2 1.13 g/ml 1.07 g/ml 1.01 g/ml Trial 3 1.11
More informationUnit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
More informationChemistry 30: Thermochemistry. Practice Problems
Name: Period: Chemistry 30: Thermochemistry Practice Problems Date: Heat and Temperature 1. Pretend you are doing a scientific study on the planet Earth. a. Name three things in the system you are studying.
More informationc. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
More information1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %
1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16
More informationChemistry Final Exam: Practice Problems
Chemistry Final Exam: Practice Problems 1. Key Vocabulary/Terms: atomic number element compound kinetic theory acid base salt vaporization condensation evaporation boiling sublimation energy level valence
More informationChapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
More information(a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
More information2 nd Semester Study Guide 2017
Chemistry 2 nd Semester Study Guide 2017 Name: KEY Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationAP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry
AP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry STP 1. What is standard pressure for each of the following: atm, mm Hg, Torr, kpa, PSI 2. Convert each of the following: a. 700 mm Hg to
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationFINAL EXAM REVIEW I will provide all of the same sheets I provided on the quizzes this semester.
Name: Class: Date: FINAL EXAM REVIEW I will provide all of the same sheets I provided on the quizzes this semester. True/False Indicate whether the statement is true or false. 1) Colligative properties
More information1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O
Pre-AP Chemistry Spring 2016 Final Review Objective 6.1: Students will recognize indicators of chemical change write balanced chemical equations to describe them based on common reactivity patterns. [S.12.C.1,
More informationChapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes and Aqueous Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component that does
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting
More informationChemistry 20 Lesson 36 The Whole Enchilada
Unit I: Science 10 Review Chemistry 20 Lesson 36 The Whole Enchilada 1. Classify the substances as ionic (i), molecular (m), or acid (a) and provide the IUPAC name and the state of matter at SATP where
More informationUnit Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
More informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
More informationBalancing Equations Notes
. Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
More informationNet Ionic Reactions. The reaction between strong acids and strong bases is one example:
Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you
More informationSlide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date»
Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
More information4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4
Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react
More informationAP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry
I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the
More informationUNIT 1 Chemical Reactions Part II Workbook. Name:
UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) When the following equation is balanced, the coefficients are. 1) NH3 (g) + O2 (g) NO2
More informationName Date Class THE ARITHMETIC OF EQUATIONS
12.1 THE ARITHMETIC OF EQUATIONS Section Review Objectives Calculate the amount of reactants required or product formed in a nonchemical process Interpret balanced chemical equations in terms of interacting
More informationEvidence of a chemical reaction: heat, light, sound, gas emitted, color change, odor
Unit 7: Chemical Equations Evidence of a chemical reaction: heat, light, sound, gas emitted, color change, odor A reaction has occurred if the chemical and physical properties of the reactants and products
More informationChapter 04. Reactions in Aqueous Solution
Chapter 04 Reactions in Aqueous Solution Composition Matter Homogeneous mixture Contains One visible distinct phase Uniform properties throughout Two or more substances that are mixed together Substances
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More informationUnit 4. Multiple Choice Identify the choice that best completes the statement or answers the question.
Unit 4 Multiple Choice Identify the choice that best completes the statement or answers the question. 39. Changing a subscript in a correctly written chemical formula a. changes the number of moles represented
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More informationAP Chemistry Semester 1 Practice Problems
AP Chemistry Semester 1 Practice Problems 1. Adipic Acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a) C 3 H 5 O 2 b) C 3 H 3 O 4 c) C 2 HO 3 d) C 2 H 5 O 4 e) C 3
More information8. A piece of Mg(s) ribbon is held in a Bunsen burner flame and begins to burn according to the equation: 2Mg(s) + O2 (g) 2MgO(s).
1. Which event must always occur for a chemical reaction to take place? A) formation of a precipitate B) formation of a gas C) effective collisions between reacting particles D) addition of a catalyst
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
941_2nd Exam_941117 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) If the heat capacity of a ceramic cup is 0.820 J C-1, how much heat is required
More information