Regents Chemistry Reference Table Review Exercises

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1 Regents Chemistry Reference Table Review Exercises Use your reference tables to answer all of the questions that follow TABLE A What do the letters STP stand for? Define the values for STP. What is the volume of a gas at 150 kpa if it occupied 2.50 L at standard pressure and constant temperature? (show your work!) What is the volume of oxygen gas at STP if it occupies 56.0 ml of volume at 52 ºC and 1.58 atm of pressure? (show your work!) Standard Temperature and Pressure 273 K -or- 0 ºC kpa -or- 1 atm use Boyle s Law: P1V1 = P2V2 V2 = P1V1 / P2 V2 = (101.3 kpa)(2.50 L) / (150 kpa) V 2 = 1.68 L use the Combined Gas Law: Kelvin!) V2 = P1V1T2 / P2 T1 (temp must be in V2 = (1.58 atm)(0.056 L)(273 K) / (1 atm)(325 K) V 2 = L = 74 ml TABLE B At 100 ºC liquid water will vaporize into its gaseous form. How much energy is necessary to evaporate one mole of liquid water at its boiling point? (show your work!) Why is the value for a substance s molar heat of vaporization so much higher than its value for molar heat of fusion? Explain! use Heat of Vaporization relationship: q = mhv q = (18 g H2O)(2260 J/g) q = joules Solids and liquids are condensed phases, while gases are not. As a result, it takes much more energy to separate the connected particles of a liquid into a gas, as opposed to (just slightly) separating the connected particles of a solid into the connected particles of a liquid. How much heat energy does it take to melt 5.0 grams of ice? (show your work!) How much heat energy does it take to warm 5.0 grams of water from 15 ºC to 28 ºC? (show your work!) use Heat of Fusion relationship: q = mhf q = (5.0 g H2O)(334 J/g) q = 1670 joules use heat transfer relationship: q = mcδt q = (5.0 g H2O)(4.18 J/g K)(13 K) q = joules TABLE C How many grams are in 1 kilogram? 1 kg = 1000 g

2 Convert 1 liter to milliliters using exponential notation 1 L = 1000 ml = 1 x 10 3 ml 45 km = 45,000 m = 4,500,000 cm (1 m How many centimeters is 45 km? = 100 cm) TABLE D What does the symbol Pa stand for and what quantity does it represent? the Pascal; it represents pressure (force per unit area) Convert 50 ºC to Kelvin. Name 2 units that define concentration. What unit quantifies amount of heat? 50 ºC = 323 K molarity (mol per liter); parts per million (ppm) the joule TABLE E What is the correct chemical formula for sodium thiosulfate? Write the correct chemical formula for each of the following: ammonium sulfate lead (II) chromate potassium dichromate silver nitrate aluminum hydroxide What is the correct name for the substance with the formula NH4SCN? What is the name of the calcium salt of sulfuric acid? Na2S2O3 (NH4)2SO4 PbCrO4 K2Cr2O7 AgNO3 Al(OH)3 ammonium thiocyanate calcium sulfate TABLE F State whether each of the following compounds are soluble or insoluble: sodium phosphate silver chloride lead (II) sulfate iron (III) hydroxide soluble insoluble insoluble insoluble Which, if any, of the compounds at 1) sodium nitrate 3) lead (II) chloride right will readily dissolve in water? 2) calcium carbonate 4) iron (II) hydroxide Which, if any, of the compounds at 1) AgHCO3 3) AgNO3 right will not readily dissolve in water? 2) AgSO4 4) AgClO3 What will most likely occur upon 1) no precipitate forms 3) CaS precipitates out

3 mixing aqueous solutions of (NH4)2S and CaBr2? 2) NH4Br precipitates out 4) CaBr2 precipitates out TABLE G True of False? as temperature of the solvent increases, the solubility of NH3 increases at 50 ºC, the saturation point for NaCl is about 30 g per 100 g of water a solvent is the substance added to a solute 120 g of KI at 10 ºC forms a saturated solution 100 g of water is the same as 100 ml of water true at 30 ºC, 100 g of NaNO3 will saturate 200 ml of water Which quantity at right will form a saturated solution of 100 g of water at 45 ºC? 1) 30 g of KCl 3) 60 g of KNO3 2) 35 g of NH4Cl 4) 110 g of NaNO3 A solution contains 90 g of KNO3 in 100 g of water at 50 ºC. The solution is 1) dilute and unsaturated 3) concentrated and unsaturated considered to be 2) dilute and supersaturated 4) concentrated and supersaturated TABLE H What is the vapor pressure of ethanol at 50 ºC? 30 kpa If the current atmospheric pressure is 50 kpa, at what temperature (in ºC) will water boil? 82 ºC What is the boiling point of ethanol at standard pressure? 80 ºC Why does propanone have a higher overall vapor pressure and lower boiling point at standard conditions The intermolecular forces of than the other substances on the table? Be specific! attraction in propanone are weaker than in the other substances, therefore, the molecules in propanone will separate and vaporize at a lower temperature than the other liquids will. TABLE I The production of which of the 1) hydrogen iodide 3) nitrogen dioxide substances at right is exothermic? 2) carbon dioxide 4) ethene How much energy is released by the 1) 3351 kj 3) 6702 kj formation of one mole of Al2O3? 2) 1676 kj 4) kj When KNO3(s) is dissolved in water, the temperature of the water will 1) increase 3) remain the same 2) decrease It takes How much heat is required to form one mole of NO(g) out of its component elements? kj to form two moles of NO(g) (see chart), therefore it will only take 91.3 kj to form one mole of NO(g).

4 If a reaction has a negative value for ΔH, how does the enthalpy of the products compare to the enthalpy of A negative value of ΔH indicates an exothermic reaction. This means the reactants? that the enthalpy of the reactants is greater than the enthalpy of the products, causing the difference to be released in the form of heat. (There is more stored energy in the reactants than in the products.) TABLE J Electrochemically, which would be a 1) Au 3) Ti good metal to use to fill teeth? 2) Zn 4) Fe Which halogen is least reactive? 1) F2 3) Br2 2) Cl2 4) I2 Lithium and fluorine are combined in a reaction chamber. Write the half-reactions for the oxidation and reduction processes that result. Will Ba 0 react with Mn 2+? Will Na + react with Cr 0? oxidation: Li 0 Li e reduction: F e 2 F 1 yes (it is higher up, therefore more likely to lose e ) no (it is higher up, therefore less likely to gain e ) What are the products of the reaction Mg 0 + Co(NO3)2? +? Mg(NO3)2 + Co 0 TABLE K What is the correct formula for phosphoric acid? H3PO4 Copper will react with this acid to produce blue copper ions, and a 1) hydrochloric acid 3) sulfuric acid reddish-brown gas. 2) nitric acid 4) phosphoric acid TABLE L The reaction of sodium metal and 1) H2 and KOH 3) Ca(OH)2 and H2O water yields which of the following? 2) H2O and NaOH 4) NaOH and H2 Write the equation for the reaction between ammonia and water. Identify the Brønsted-Lowry acids and bases. Identify the conjugate acid-base pairs. base acid acid base NH3 + H2O = NH4 + + OH TABLE M Which indicator(s) would you use to identify the following: a strong acid? a weak acid? a strong base? a weak base? methyl orange bromcresol green phenolphthalein thymol blue

5 What color is phenolphthalein in a solution whose ph is 11? pink Thymol blue would be yellow in what ph solution? ph of 8.0 or lower Which indicator(s) would be best for an acid-base titration whose equivalency point is a ph of 6.5? bromthymol blue TABLE N An alpha particle is the same as a 1) hydrogen nucleus 3) hydrogen atom 2) helium nucleus 4) helium atom If Fr-220 undergoes alpha decay, what 1) At-216 3) At-85 is the daughter nuclide? 2) At-220 4) At-83 If you start with 1000 grams of Au-198, how much of it will remain after 7 half-lives? How much time will this take? grams would remain 2.69 days x 7 = days total time What is the number of hours required for potassium-42 to undergo 3 half-life 1) 6.2 hours 3) 24.8 hours periods? 2) 12.4 hours 4) 37.2 hours How many grams of a 64 gram sample of 32 P will remain after 71.5 days 1) 2 grams 3) 8 grams elapses? 2) 4 grams 4) 16 grams TABLE O Write the notation for each of the following: proton alpha particle -or- -or- neutron beta particle -or- Which two particles have approximately 1) neutron & electron 3) proton & neutron the same masses? 2) neutron & deuteron 4) proton & electron Which nuclear emission moving through an electric field would be deflected 1) an alpha particle 3) gamma rays toward the positive electrode? 2) a beta particle 4) a proton Which particle is electrically neutral? 1) a proton 3) a neutron 2) a positron 4) an electron Write the transmutation equation for the decay of cobalt-60. A gamma ray is electromagnetic What is the difference between a gamma ray and a beta particle? radiation with an extremely small wavelength and therefore a very high frequency; it has very great penetrating power. A beta emission is actually a particle, equivalent to an electron, and has much less penetrating power.

6 TABLES P & Q What is the correct chemical formula for propane? Which homologous series of hydrocarbons is saturated? C3H8 the alkane series What is the correct IUPAC name for the following hydrocarbon? H H H C C C C C C C C H Tables P & Q, continued What is the name of the compound with the formula C4H6? What is the correct IUPAC name for each of the following hydrocarbons? H C C C H n-octene (or, 1- octene) propane butyne H H C C C C H H H H H H C C C C C C C H H H 2-butene 3-heptyne TABLE R Identify each of the following organic functional groups: R COO R OH R CHO R CO R COOH ester alcohol aldehyde ketone organic acid Name each of the following chemical compounds: CH3CH2CH2C=O OH butanoic acid CH3C=OCH3 propanone (acetone) CH3CH2OH ethanol What is the correct IUPAC name for each of the following compounds? H C C C C O H H O H H C C C C C H H H butanal 2-pentanol

7 H H Br Br H H C C C C C H H H 2,3-dibromopentane PERIODIC TABLE ethylamine Matching f 3/4 of the elements are classified as these a) diatomic molecules q the weighted average mass of all isotopes of that element b) noble gases b these elements are considered chemically inert c) halogens y has 3 valence electrons d) alkaline earth metals s term describing a horizontal row e) alkali metals o this element forms the basis of organic compounds f) metals n these elements sit on the step ladder g) nonmetals m is a nonmetal liquid at room temperature h) carbon-12 a Br2I2N2Cl2H2O2F2 i) ionization energy k F has a very high value due to its attraction for electrons j) transition metals x the electron configuration for an ion of calcium k) electronegativity h relative atomic masses are based on this element l) mercury r the elements in this grouping are physically and chemically related m) bromine d barium is within this group n) metalloids p forms a tetrahedral unit which is the basis of sand and rocks o) carbon t the Periodic Table is arranged according to this p) silica j form colored ions in solution q) atomic mass l is the only liquid metal at normal conditions r) family c form negative ions, are very reactive, form ionic solids with alkali metals s) period i increases from left to right across a period t) atomic number g elements in the upper right corner of the Periodic Table u) plutonium e soft, highly reactive metals, rarely found in nature uncombined v) atomic size w electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 w) v decreases from left to right across a period x) u is a radioactive, fissionable material y) gallium TABLE S Define each of the following terms: the amount of energy necessary to remove an electron from an ionization energy atom in the ground state electronegativity H C C N a(n arbitrary) measure of an atom s ability to attract electrons while in a chemical bond with another atom the temperature at which the vapor pressure above a liquid equals boiling point the atmospheric pressure pushing down on the liquid s surface Which element has the highest electronegativity? fluorine

8 Which element has the highest ionization energy? How many meters is the radius of a hydrogen atom? Which element has the largest atoms? Name each of the following elements: helium 37 pm = 3.7 x m 1) sulfur 3) potassium 2) chlorine 4) calcium Hg mercury Sn tin Ge germanium Fe iron Mo molybdenum Sb antimony W tungsten K potassium TABLE T 500 K is equivalent to how many ºC? 1) 227 ºC 3) 773 ºC 2) ºC 4) 1000 ºC How many moles are contained in a 1) 0.30 mol 3) 150 mol 500 ml sample of a 0.3 M solution? 2) 0.15 mol 4) 300 mol What is the percent composition by mass of carbon in CH3COOH? 1) 3) 2) 4) How many moles of Al(OH)3 exist in 1) 2.56 mol 3) 7.69 mol 200 grams of it? 2) 1.28 mol 4) 22.4 mol Two moles of an unknown gas at STP have a mass of 10 grams. What is the density of the gas? What is the molarity of 25 ml of an acid (monoprotic) if it is exactly neutralized by mixing it with 75 ml of 0.1 M NaOH? 1) 20 g/l 3) 40 g/l 2) 0.44 g/l 4) 0.22 g/l 1) 0.3 M 3) 0.15 M 2) 0.6 M 4) 3 M use heat transfer relationship: What is the final temperature, in Kelvin, of the water in a calorimetry reaction in which 2000 joules of heat are absorbed by the water? The initial temperature of the water is 100 ºC and it has a mass of 30 grams. (show your work!) q = mcδt Δt = 15.9 K = 15.9 ºC Δt = tf ti tf = Δt + ti tf = 100 ºC ºC tf = ºC = K use percent error relationship: A student s experiment shows the volume of 1.00 mole of gas at STP to be 26.3 L. What is the student s percent error from the accepted value? (show your work!) % error = 17.4 %

9 use parts per million relationship: How many grams of a salt must be in 500 grams of solution to have a concentration of 100 ppm? (show your work!) solve for x x =.05 grams

4. How much heat does it take to melt 5.0 g of ice? 5. How many grams of water can 10. kj boil into vapor?

4. How much heat does it take to melt 5.0 g of ice? 5. How many grams of water can 10. kj boil into vapor? REFERENCE TABLE REVIEW Since reference table are used so often by scientists and students of science, it is appropriate that high school chemistry students be familiar with them. The tables provided by