A201. Milwaukie HS Chemistry Herrington/Linman. Period Date / / Balance the following Chemical Reactions 1. H 2 + O 2 H 2 O

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1 A201 Balance the following Chemical Reactions 1. H 2 + O 2 H 2 O 2. Ca 3 (PO 4 ) 2 + H 2 SO 4 CaSO 4 + Ca(H 2 PO 4 ) 2 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C + HCl 7. Si 2 H 3 + O 2 SiO 2 + H 2 O 8. Fe + O 2 Fe 2 O 3

2 A202 Group Assignment Balance the following equations: 1. Zn (s) + AgNO 3 (aq) Zn(NO 3 ) 2 (aq) + Ag (s) 2. N 2 (g) + H 2 (g) NH 3 (g) 3. NaCl (aq) + AgC 2 H 3 O 2 (aq) NaC 2 H 3 O 2 (aq) + AgCl (s) 4. Mg(OH) 2 (aq) + H 3 PO 4 (aq) H 2 O (l) + Mg 3 (PO 4 ) 2 (aq) 5. HNO 3 (aq) + Ni (s) Ni(NO 3 ) 2 (aq) + H 2 (g) 6. H 3 PO 4 + (NH 4 ) 2 MoO 4 + HNO 3 (NH 4 ) 3 PO 4. MoO 3 + NH 4 NO 3 + H 2 O

3 A203 Group Assignment Balance the following equations: 1. Propane(C3H8) is burned in air to form carbon dioxide and water. 2. Hydrogen sulfide gas is bubbled into a solution of mercury(ii) chloride to mercury(ii) sulfide and hydrochloric acid. 3. Solid lithium oxide is added to excess water to form lithium hydroxide solution. 4. Phosphoric acid is decomposed into elements. 5. Tin(II) oxide is made from its elements.

4 CA 201 Computer : Balancing One

5 CA 202 Computer : Balancing Two

6 Lab201 Reaction Types OBJECTIVES: In this assignment, you will perform four types of chemical reactions; identify some products of the reactions; and, write and balance equations for the reactions observed. CHEMICALS: 6 M HCl 0.1 M K2CrO4 magnesium lime water( identifies CO2 gas) zinc pieces copper(ii) carbonate PRECAUTIONS: goggles, tie long hair and apron PROCEDURE: A. SYNTHESES REACTION: 1. Place a loosely rolled-up strip of magnesium in a clean dry crucible. Find the mass of the crucible and magnesium to two places beyond the decimal. Record the mass in table a. Table a a Mass of Crucible Empty g b Mass of Crucible and Magnesium g c Mass of Crucible and product after Heating. g d Mass of Magnesium(b minus a) e Product mass after heating.(c minus a) g 2. Place the crucible containing the magnesium on the ring stand as in figure a. 3. Heat the crucible, gently at first, until the crucible bottom becomes red hot for for ten minutes. (DO NOT LOOK AT THE BURNING MAGNESIUM.) 4. Describe the results of heating the magnesium. 5. Find the total mass of the crucible and product after heating. Record the mass in table a. figure a 6. Predict formulas for the product based on ions from your cation/anion chart and the fact that oxygen gas and nitrogen gas from the air reacted with the heated magnesium. magnesium nitride: magnesium oxide: 7. Add a few drops of water to the product. Smell the damp product. What odor did you detect? Clean out the crucible into the waste bucket. Put the crucible back where it belongs Observations: 8. Write the two reactions observed: one for magnesium reacting with nitrogen to form magnesium nitride and one for magnesium reacting with oxygen to form magnesium oxide.. 1) Word Equation + Balanced Equation + 2) Word Equation + Balanced Equation +

7 B. DOUBLE DISPLACEMENT REACTION: 1. To one small test tube add 5 drops of potassium chromate. 2. To the same test tube add about 5 drops of silver nitrate. 3. Describe the reaction which occurred. 2. Write the reaction which occurred. Word Equation + + Balanced Equation + + C. SINGLE DISPLACEMENT REACTION: 1. Clean and dry the equipment. Set it up as in the figure c. figure c. 2. Add to the test tube 2 to 3 ml of HCl(aq). 3. Put a piece of zinc into the acid and assemble the apparatus. 4. Collect the gas generated by the reaction. This may take several minutes.(do NOT HEAT THE ACID.) 5. While still holding the gas collecting tube inverted, insert a burning splint into the inverted test tube. Observations: 6. Write the reaction which occurred when zinc reacts with acid. Word Equation + + Balanced Equation + + D. DECOMPOSITION REACTION: 1. Set up the apparatus as in figure b. figure b 3. Place two small spatulas of copper(ii) carbonate in the test tube containing the stopper. 4. Add to the test tube 2 to 3 ml of lime water. Limewater turns milky white in the presence of carbon dioxide. 4. Make sure the cork is tight.then gently heat the test tube containing the copper(ii) carbonate. 5. Describe the change in the lime water as the gas from the heated test tube bubbles into the lime water. Pull the rubber tube out of the lime water before turning off the burner. Observations:

8 6. Write the reaction which occurred when copper(ii) carbonate decomposed to form copper(ii) oxide and carbon dioxide. Word Equation + Balanced Equation + CONCLUSIONS AND QUESTIONS: 1. Why did the mass increase during the burning of the magnesium in part A? 2. What is the difference between a physical reaction and a chemical reaction? 3. Identify each equation as one of the four reaction types(syn, DEC, SD or DD) studied in the laboratory. type: Mg(s) + 2HCl(aq) > MgCl2(aq) + H2(g) type: 4Fe(c) + 3O2(g) -----> 2Fe2O3(c) type: 2Ag2O(c) -----> 4Ag(c) + O2(g) type: Ca(OH)2(aq) + H2SO4(aq) -----> CaSO4(c) + 2H2O(l) type: Cu(c) + 2AgNO3(aq) -----> Cu(NO3)2(aq) + 2Ag(c)

9 A204 Reaction Types: Writing and Balancing 1. Dilute sulfuric acid is added to a solution of barium acetate. 2. Ammonium chloride crystals are added to a solution of sodium hydroxide. 3. A precipitate is formed when solutions of trisodium phosphate and calcium chloride are mixed. 4. Equal volumes of 0.1 M hydrochloric acid and 0.1 M disodium hydrogen phosphate are mixed. 5. Hydrogen sulfide gas is bubbled through a solution of lead(ii) nitrate. 6. Solutions of silver nitrate and sodium chromate are mixed. 7. Solutions of sodium fluoride and dilute hydrochloric acid are mixed. 8. A saturated solution of barium hydroxide is mixed with a solution of iron(iii) sulfate. 9. A solution of ammonium sulfate is added to a potassium hydroxide solution. 10. A solution of ammonium sulfate is added to a saturated solution of barium hydroxide.

10 A205 Balancing Equations Race

11 A206 Writing Reactions Write a balanced equation based on the descriptions of chemical reactions below. You will need your ion chart to write some of the chemical formulas. 1. Many people keep hydrogen peroxide (H 2 O 2 ) on hand in their homes for use as an antiseptic (to kill germs in minor cuts). Hydrogen peroxide is unstable, and it decomposes to produce oxygen gas and water. 2. If clear solutions of sodium iodide and lead (II) nitrate are mixed, bright yellow lead (II) iodide will precipitate, leaving a solution of sodium nitrate. 3. Nitrous oxide (N 2 O), also known as "laughing gas" is used by some dentists as an anesthetic. Nitrous oxide (and water vapor as a by-product) can be produced in small quantities in the laboratory by careful heating of solid ammonium nitrat 4. Hydrogen sulfide gas (H 2 S) is responsible for the odor of rotten eggs. Hydrogen sulfide burns with oxygen in the air, producing sulfur dioxide gas (SO 2 ) and water vapor. 5. When a strip of magnesium metal is dropped into an orange solution of iron (III) nitrate (ferric nitrate), solid iron precipitates, leaving a clear solution of magnesium nitrate. 6. A common demonstration in general chemistry courses is the "volcano" reaction. When ammonium dichromate is heated, it decomposes into chromium (III) oxide, nitrogen gas, and water vapor.

12 A207 Six Types of Chemical Reactions Balance the following reactions and indicate which of the six types of chemical reaction are being represented: 1) NaBr + Ca(OH) 2 --> CaBr 2 + NaOH Type of reaction: 2) NH 3 + H 2 SO 4 --> (NH 4 ) 2 SO 4 Type of reaction: 3) C 5 H 9 O + O 2 --> CO 2 + H 2 O Type of reaction: 4) Pb + H 3 PO 4 --> H 2 + Pb 3 (PO 4 ) 2 Type of reaction: 5) Li 3 N + NH 4 NO 3 --> LiNO 3 + (NH 4 ) 3 N Type of reaction: 6) HBr + Al(OH) 3 --> H 2 O + AlBr 3 Type of reaction: 7) What s the main difference between a double displacement reaction and an acid-base reaction? 8) Combustion reactions always result in the formation of water. What other types of chemical reaction may result in the formation of water? Write examples of these reactions below.

13 A208 Word Equations Write the word equations below as chemical equations and balance: 1) Zinc and lead (II) nitrate react to form zinc nitrate and lead. 2) Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas. 3) Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride. 4) Potassium metal and chlorine gas combine to form potassium chloride. 5) Aluminum and hydrochloric acid react to form aluminum chloride and hydrogen gas. 6) Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. 7) Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide. 8) Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas.

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