START HERE FOR CHEM B 146. The gram molecular mass of oxygen is ____.

a) 16.0 g b) 32.0 g c) equal to a mole of oxygen atoms d) none of the above 147. What is the mass in grams of 5.90 mol C8H18? a) 0.0512 g b) 19.4 g c) 389 g d) 673 g e) 3.55 x 1024 g

148. What is the number of moles in 0.025 g (NH4)2Cr2O7? a) 7.2 x 104

b) 1.1 c) 6.02 x 1023

d) 110 e) none of these

149. A 22.4 L sample of which of the following substances, at STP, would contain 6.02 x 1023

representative particles? a) oxygen b) gold c) cesium iodide d) sulfur e) all would have the same number of representative particles.

150. Which of the following gas samples would have the largest number of representative particles at STP? a) 12.0 L He b) 7.0 L O2 c) 0.10 L Xe d) 0.007 L SO3 e) 5.5 L N2O

Page 26

151. What is the volume, in liters, of 0.750 mol of C3H8 gas at STP?

a. 0.0335L b) 16.8 L c) 29.9L d) 739L e) 1310 L

146) B 147) D 148) E 149) A 150) A 151) B

152. What is the number of moles in 500 L of He gas at STP? Watch significant digits! a) 0.05 mol b) 0.2 mol c) 20 mol d) 90 mol e) 10,000 mol

153. How many moles of Ar atoms are there in 202 L of Ar gas at STP? a) 1.20 x 1024 mol b) 4.52 x 103 mol c) 9.02 mol d) 1.79 mol e) 1.11 x 10-1 mol

154. If the density of an unknown gas Z is 4.50 g/L at STP, what is the gram formula mass of gas Z? a) 0.201 g b) 5.00 g c) 26.9 g d) 101 g e) This cannot be determined without knowing the formula of the gas.

155. If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent composition of Hg in the compound? a) 28. 5% b) 39.9% c) 71.5% d) 60.1% e) 251%

156. What is the mass of silver in 3.4 g AgNO3? a) 0.025 g b) 0.032 g c) 0.64 g d) 2.2 g e) 3.0 g

157. All of the following are empirical formulas EXCEPT ____. a) Na2SO4

b) C6H5Cl c) N2O4

d) Sn3(PO4)4

152) C 153) C 154) D 155) C 156) D 157) CPage 27

158. What is the empirical formula of a compound that is 50.7% antimony and 49.3% selenium by weight? a) SbSe b) SbSe2 c) Sb2Se d) Sb2Se3 e) Sb3Se2

159. The coefficients are missing from the skeleton equation below. NH3(g) + O2 N2(g) + H2O(l)

The correct order of the missing coefficient is ___. a) 4, 3, 2, 6 b) 2, 1, 2, 3 c) 1, 3, 1, 3 d) 3, 4, 6, 2

160. Write a balanced equation for sodium and iodine reacting to make sodium iodine. Then state what the coefficient and symbol for iodine will be in that reaction. a) 2I- b) I c) 2I

d) I2 e) 2I2 161. Write a balanced equation for the combination reaction that takes place when iron(III) oxide is formed from it constituent elements.

a) Fe2+O3 Fe2O3

b) 2Fe +3O Fe2O3 c) 4Fe +3O2 2Fe2O3 d) 3Fe +O Fe3O e) Fe+O3 FeO3

162. In order for the reaction 2Al +6HCL 2AlCl3 +3H2 (g) to occur, which of the following must be true?

a) Al must be above Cl on the activity series. b) Al must be above H on the activity series. c) Heat must be supplied for the reaction d) A gas must be formed. 158) D 159) A 160) D 161) C 162) B Page 28

163. A double replacement reaction takes place when aqueous cobalt(III) chloride reacts with double aqueous lithium hydroxide. One of the products of this reaction would be____. a) Co(OH) 3 b) Co(OH) 2 c) LiCo3 d) LiCl3 e) Cl3OH

164. The products of a combustion reaction do NOT include _____. a) Water b) Carbon dioxide c) Carbon monoxide d) Heat e) Hydrogen

165. In every chemical reaction. _____. a) Mass and molecules are conserved b) Moles and liters are conserved c) Mass and atoms are conserved d) Moles and molecules are conservede) Mass and liters are conserved

166. What volume does 1 mole of gas particles occupy at STP? a) 1 L b) 2.4 L c) 10 L d) 22.4 L e) 100 L

167. What is the volume occupied by 1.5 mol of hydrogen at STP? a) 11.2 L b) 22.4 L c) 33.6 L d) 44.8 L e) 56. L 163) A 164) E 165) C 166) D 167) C Page 29 168. Which of the following statements is true about the total number of reactants and the total number of products in this reaction? C5H12 (I) + 8 O2 (g) 5 CO2 (g) + 6 H2O (g) a) 9 moles of reactants regroup to form 11 moles of product b) 9 grams of reactants regroup to form 11 grams of product c) 9 liters of reactants regroup to form 11 liters of product d) 9 atoms of reactants regroup to form 11 atoms of product e) 22.4 liters of reactants regroup to form 22.4 liters of product

169. How many moles of aluminum are needed to react completely with 1.8 mol of FeO?

2Al(s) + 3FeO(s) 3Fe(s) + Al2O3(s) a) 0.9 mol b) 1.2 mol c) 1.8 mol d) 2.7 mol e) 3.6 mol

170. How many moles of glucose, C6H12O6, can be “burned” biologically when 10.0 mol of oxygen is available? C6H12O6 + 6 O2 6 CO2 + 6 H2O a) 0.938 mol b) 1.67 mol c) 53.3 mol d) 60.0 mol e) 301 mol

171. When glucose is consumed it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C6H12O6 completely reacted with oxygen? C6H12O6 + 6 O2 6 CO2 + 6 H2O a) 1.5 g b) 1.8 g c) 11 g d) 66 g e) 12,000 g

172. How many moles of H3PO4 are produced when 71.0 g P4O10 reacts completely to form H3PO4?

P4O10(s) + 6H2O(l) 4H3PO4(aq) a) 0.0635 mol b) 1.00 mol c) 4.00 mol d) 16.0 mol e) 98.0 mol

168) A 169) B 170) B 171) D 172) B Page 30

173. How many liters of NH3, at STP, will react with 5.3 g O2 to form NO2 and water

4NH3(g) + 7O2(g) 4NO2 + 6H2O(g) a) 0.002423 L b) 2.12 L c) 3.03 L d) 6.49 L e) 77.3 L

174. Identify the limiting reagent and the volume of product formed when 11 L CS2 reacts with 18 L O2 to produce CO2 gas and SO2 gas at STP.

CS2(g) + 3O2(g) CO2(g) + 2SO2(g) a) CS2 ; 5.5 L CO2

b) O2 ; 6.0 L CO2

c) CS2 ; 11 L CO2

d) O2 ; 27 L SO2

e) O2 ; 54 L CO2

175. Heating can decompose lead nitrate. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO3)2 is heated to give 5.5 g of PbO?

2Pb(NO3)2(s) 2PbO(s) + 4NO2(g) +O2(g) a) 18 % b) 44% c) 56% d) 67% e) 82%

176. Equal volumes of nitrogen and oxygen, at the same temperature and pressure, would ____. a) have the same mass b) contain the same number of particles c) contain different numbers of particles d) have different average kinetic energies

177. What happens to the temperature of a liquid as it evaporates? a) It increases b) It decreases c) It does not change

178. An increase in the temperature of a contained liquid ____. a) has no effect on the kinetic energy of the liquid b) decreases the vapor pressure of the liquid c) causes fewer particles to escape the surface of the liquid d) causes the vapor pressure above the liquid to increase

173) B 174) B 175) E 176) B 177) B 178) D Page 31

179. When the external pressure is 505 kPa, what is the vapor pressure of water at its boiling point? a) 0 kPa b) 101 kPa c) 505 kPa d) 1010 kPa

180. Water could be made to boil at 105°C instead of 100°C by ___. a) applying a great deal of heat b) increasing the air pressure on the water c) decreasing the pressure on the water d) decreasing the air pressure above the water

181. The boiling points of ionic solids tend to be ____. a) low b) high c) average

182. Which of the following is NOT a phase change? a) sublimation b) melting c) diffusion d) vaporization

183. Which of the following has the greatest heat capacity? a) 1,000 g of water b) 1,000 g of steel c) 1 g of water d) 1 g of steel

184. What is the amount of heat required to raise the temperature of 100 g of aluminum by 10°C? (specific heat of aluminum = 0.21 cal /g x °C a) 0.21 cal b) 2.1 cal c) 210 cal d) 21,000 cal e) None of the above

185. When cooking with natural gas, the energy comes form ____. a) kinetic energy in the gas b) chemical potential energy of the gas molecules c) the pressure of the gas d) the volume of the gas

179) C 180) B 181) B 182) C 183) A 184) C 185) BPage 32

186. Two objects are sitting next to each other in direct sunlight. Object A gets hotter than object B. a) Object A has a higher specific heat than object B. b) Object A has a lower specific heat than object B. c) Both objects have the same specific heat.

187. Compared to 100 g of iron, a 10-g sample of iron has ____. a) a higher specific heat b) a lower specific heat c) the same specific heat

188. If the heat involved in a chemical reaction has a negative sign, ____. a) heat is lost to the surroundings b) heat is gained from the surroundings c) no heat is exchanged in the process

189. If you were to touch the flask in which an endothermic reaction were occurring, ____. a) the flask would probably feel cooler than before the reaction started b) the flask would probably feel warmer than before the reaction started c) the flask would feel the same as before the reaction started d) None of the above

190. The symbol “ΔH” stands for ____. a) the specific heat of a substance b) the heat capacity of a substance c) the change in heat of reaction for a chemical reaction d) one Calorie given off by a reaction

191. The following equation shows the reaction that occurs when nitroglycerine explodes.

4C3H5O9N3 12CO2 + 6N2 + O2 + 10H2O + 1725 kcal This reaction is ____. a) endothermic b) exothermic c) a combination reaction d) a combustion reaction

192. The amount of heat absorbed by a melting solid _____the amount of heat lost by a solidifying liquid. a) Is the same as b) Is less than c) Is greater than

186) B 187) C 188) A 189) A 190) C 191) B 192) APage 33

193. The vaporization of a liquid is an _____. a) Exothermic process b) Endothermic process

194. What is the standard heat of reaction for this reaction:

Zn(s) + Cu2 + (aq) Zn2 + (aq) +Cu(s) (ΔHto for Cu2 = +64.4 kJ/mol; ΔHto for Zn2 + = -152.4 kJ/mol; ΔHto for Zn= 0 kJ/mol; ΔHto for Cu = 0 kJ/mol ) a) -216.8 kJ per mole b) -88.0 kJ per mole c) 88.0 kJ per mole d) 216.8 kJ per mole

195. For a given substance, the molar heat of fusion ____ the molar heat of vaporization. a) Always equals b) Is less than c) Is greater than

196. When snow melts, what happens to the surrounding air? a) It gets warmer b) It gets cooler c) Nothing happens to the surrounding air

197. If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change within the container? a) The pressure will be twice as great b) The pressure will be four times as great c) The pressure will be five times as great d) The pressure will not change

198. Increasing the volume of a given amount of gas at constant temperature causes the pressure to decrease because ____. a) The molecules are striking a larger area with the same force b) There are fewer molecules c) The molecules are moving more slowly d) There are more molecules

199. What happens to the temperature of a gas when it is compressed a) The temperature increases b) The temperature does not change c) The temperature decreases

193) B 194) A 195) B 196) B 197) C 198) A 199) APage 34

200. What happens to the pressure of a gas inside a container if the temperature of the gas is lowered? a) The pressure increases b) The pressure does not change c) The pressure decreases

201. As the temperature of a fixed volume of a gas increases, the pressure will____. a) vary inversely b) decrease c) be unchanged d) increase

202. Boyle’s law states that ____. a) the volume of a gas varies inversely with pressure b) the volume of a gas varies directly with pressure c) the temperature of a gas varies inversely with pressure d) the temperature of a gas varies directly with pressure

203. The volume of a gas is reduced from 4 L to 0.5 L while the temperature is held constant. The pressure of the gas ____. a) increases by a factor of four b) decreases by a factor of eight c) increases by a factor of eight d) increases by a factor of two

204. Charles’ law states that ____. a) the pressure of a gas is inversely proportional to its temperature in kelvins b) the volume of a gas is directly proportional to its temperature in kelvins c) the pressure of a gas is directly proportional to its temperature in kelvins d) the volume of a gas is inversely proportional to its temperature in Kelvin

205. A sample of gas occupies 40.0 mL at -123°C. What volume does the sample occupy at 27°C? a) 182 mL b) 8.80 mL c) 80.0 mL d) 20.0 mL

200) C 201) D 202) A 203) C 204)B 205) CPage 35

206. Which of the following is constant for 1 mol of any ideal gas? a) PVT b) PVT c) PTV d) VTP 207. If a balloon containing 1,000.0 L of gas at 50.0 °C and 101.3 kPa rises to an altitude where the pressure is 50.5 kPa and the temperature is 10.0 °C. the volume of the balloon under these new conditions would be ____. a) 401L b) 569 L c) 1760 L 208. Which of the following gases will effuse the most rapidly? a) bromine b) chlorine c) ammonia d) hydrogen e) argon

209. What is primarily responsible for the water’s ability to dissolve substances?

a) Diffusion

b) Water’s polarity

c) Ionic attractions between the ions

210. What causes water’s low vapor pressure?

a) Dispersion forces

b) Covalent bonding

c) Hydrogen-bonding

d) Ionic attractions

211. The high surface tension of water is due to the _____.’

a) Small size of water molecules

b) High kinetic energy of water molecules

c) Hydrogen bonding between water molecules

d) Covalent bonds in water molecules

206) B 207) C 208) D 209) B 210) C 211) CPage 36

212. How does the heat of vaporization of the water compare with the heat of vaporization of other liquids?

a) It is lower

b) It is about the same

c) It is higher

213. What energy change occurs when 100 g of ice melts to form 100 g of water at 0.C?

a) 8 kcal is absorbed by the ice

b) 8kcal is released by the ice

216. Which of the following substances is less soluble in hot water that cold water?

a) CO2 (g) b) NaCl (s) c) NaNO3 (s) d) KBr (s)

217. What happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid decreases? a) The solubility decreases

b) The solubility increases

c) The solubility remains the same

218. What is the number of moles of solute in 250 mL of a 0.4M solution?

a) 0.1 mol b) 0.16 mol c) 0.62 mol d) 1.6 mol e) 1 mol

212) C 213) A 214) C 215) B 216) A 217) A 218) A

Page 37

219. How many mL of 3M HCl is needed to make 300 mL of 0.1M HCl?

a) 10 mL b) 100 mL c) 90 mL d) 9 mL e) 30 mL

220. What mass of sucrose, C12H22O11, is needed to make 500 mL of 0.2 M solution?

a) 34.2 g b) 100 g c) 17.1 g d) 68.4 g

221. At what stage of a reaction does the activated complex exist? a) beginning b) middle c) end

222. Why does a catalyst cause a reaction to proceed faster? a) There are more collisions per second

b) The collisions occur with greater energy

c) The activation energy is lowered

d) There are more collisions per second and the collisions are of greater energy

#226 fix laterthe effect of lowering the temperature? a) The reaction makes more products

) The reaction makes more reactants c) The reaction is unchanged

227. What is the effect of adding more water to the following equilibrium reaction. 4 C3H5O9N3 <---> 12CO2 + 6N2 + O2 + 10H2O + 1725 kcal a) More C3H5O9N3 is made b) CO2 concentration increases c) The equilibrium is pushed in the direction of the products d) Nothing

228. If a system is left to change spontaneously, in what state will it end? a) The same state in which it began b) The state with the lowest possible energy c) The state with the maximum disorder d) The state with the lowest possible energy and the maximum amount of disorder

229. Which reaction results in greatest increase in entropy? a) A B b) A 2B c) 2A B

230. The amount of disorder in a system I measured by its______. a) Activation energy b) Entropy c) Equilibrium position d) Keq

231. Which of the following systems has the highest entropy? a) 10 ml of water at 10oC b) 10 ml of water at 50oC c) 10 ml of water at 100oC d) All have the same entropy because all are water

232. When an acid reacts with a base what compound(s) is/are formed? a) A salt only b) Water only c) Metal oxides only d) A salt and water

226) A 227) A 228) D 229) B 230) B 231) C 232) D Page 39

233. What is the name of H2SO4? a) Hyposulfuric acid b) Hydrosulfuric acid c) Sulfuric acid d) Sulfurous acid e) Hydrosulfite acid

#226 fix laterthe effect of lowering the temperature? a) The reaction makes more products

) The reaction makes more reactants c) The reaction is unchanged

227. What is the effect of adding more water to the following equilibrium reaction. 4 C3H5O9N3 <---> 12CO2 + 6N2 + O2 + 10H2O + 1725 kcal a) More C3H5O9N3 is made b) CO2 concentration increases c) The equilibrium is pushed in the direction of the products d) Nothing

228. If a system is left to change spontaneously, in what state will it end? a) The same state in which it began b) The state with the lowest possible energy c) The state with the maximum disorder d) The state with the lowest possible energy and the maximum amount of disorder

229. Which reaction results in greatest increase in entropy? a) A B b) A 2B c) 2A B

230. The amount of disorder in a system I measured by its______. a) Activation energy b) Entropy c) Equilibrium position d) Keq

231. Which of the following systems has the highest entropy? a) 10 ml of water at 10oC b) 10 ml of water at 50oC c) 10 ml of water at 100oC d) All have the same entropy because all are water

232. When an acid reacts with a base what compound(s) is/are formed? a) A salt only b) Water only c) Metal oxides only d) A salt and water

226) A 227) A 228) D 229) B 230) B 231) C 232) D Page 39

233. What is the name of H2SO4? a) Hyposulfuric acid b) Hydrosulfuric acid c) Sulfuric acid d) Sulfurous acid e) Hydrosulfite acid

234. What is the concentration of H+ in a neutral solution?

a. 10M b. 1x 10 -10 c. 1x10 -7 d. can’t be determined

235. What is the ion-product constant for water?

a) 1.0 x 10-1 M2

b) 1.0 x 10-7 M2

c) 1.0 x 10-10 M2

d) 1.0 x 10-14 M2

236. If the hydrogen ion concentration is 10-1 M, what is the nature of the solution?

a) acidic

b) alkaline

c) neutral

237. If the [H+] in a solution is 1 x 10-1 mol/L, then the [OH-] is _____.

a) 1 x 10-1 mol/L

b) 1 x 10-15 mol/L

c) 1 x 10-13 mol/L

d) cannot be determined

238. A solution in which the hydroxide-ion concentration is 1 x 10-8 M is _____.

a) acidic

b) basic

c) neutral

d) None of the above

239. Which of these solutions is the most basic?

241. If the hydroxide ion concentration s 10-10 M, what is the pH of the solution?

a) 1

b) 4

c) 7

d) 10

e) 14

242. The pH pf a solution in which [OH-] = 1 x 10-4 M is ______.

a) 4.0

b) 10.0

c) –4.0

d) –10.0

243. The pH of a solution with a concentration of 0.01 M hydrochloric acid is ___.

a) 10-2

b) 12.0

c) 2.0

d) 10-12

244. What is the pH when the hydrogen ion concentration is 2 x 10-3 M?

a) 2

b) 2.7

c) 3

d) 3.3

e) 4

245. What type of acid is nitric acid?

248. A 12.0 solution of an acid that ionizes completely in solution would be termed ____. a) Concentrated and weak

b) Strong and dilute

c) Dilute and weak

d) Concentrated and strong

249. What is the concentration of sulfuric acid if 50 mL of acid is neutralizing by 10 mL of 0.1M sodium hydroxide? a) 0.005M

b) 0.02 M

c) 0.25M

d) 0.5M

250. When iron oxide becomes iron, what type of reaction occurs? a) Oxidation

b) Reduction

c) Neutralization

d) Combination

251. In the reaction of sodium with oxygen, which atom is reduced? a) sodium

b) oxygen

c) both

d) neither

252. Identify the reducing agent in the following reaction.

2Na + S Na2S

a) Na

b) S

c) Na2S

254. What is the sum of the oxidation numbers in the phosphate ion?

a) 0

b) –1

c) –2

d) –3

e) –4

255. In the following unbalanced reaction, which atom is reduced?

H2O + Cl2 + SO2 HCl + H2SO4

a) Hydrogen

b) Oxygen

c) Chlorine

d) Sulfur

256. Which element increases its oxidation number in the following reaction?

3KOH + H3PO4 K3PO4 + 3H2O

a) potassium

b) oxygen

c) hydrogen

d) phosphorous

e) none

257. How many double covalent bonds are in alkane?

a) none

b) one

c) two

d) three

e) the number varies

258. How many valence electrons surround a carbon atom?

a) 1

267. If the half-life of a radioactive material is 8 years, how many years will it take for one half of the original amount of material to decay?

a) 2 years

b) 4 years

c) 8 years

d) 16 years

e) 32 years

268. If the half-life of a sodium-24 is 15 hours, how much remains from an 8.0 gram sample after 60 hours?

a) 0.5 grams

b) 1.0 grams

c) 2.0 grams

d) 4.0 grams

269. Which of the following particles is needed to complete this nuclear equation? 5525 Mn + 21H ---> _______ + 2 10 n

a) 5627 Co

b) 2725 Mn

c) 5526 Fe

d) 5824 Cr

270. To what element does polonium–214 decay to when it loses an alpha particle? (atomic number is 84)

a) 21082 Pb

b) 21082Po

c) 21482 Pb

d) 21482 Rn