Chemical Reactions - 5 STEPS TO A 5: 500 AP Chemistry Questions to Know by Test Day! (2012)

5 STEPS TO A 5: 500 AP Chemistry Questions to Know by Test Day! (2012)

Chapter 5. Chemical Reactions (Questions 181–230)

181. How many molecules are contained in 180 g of water (H2O)?

(A) 6.02 × 1022

(B) 1.20 × 1023

(C) 6.02 × 1023

(D) 1.20 × 1024

(E) 6.02 × 1024

182. How many oxygen atoms are in 4.4 g of CO2?

(A) 6.02 × 1022

(B) 1.20 × 1023

(C) 1.20 × 1024

(D) 6.02 × 1023

(E) 6.02 × 1024

183. How many atoms of hydrogen are in 1.5 g of ribose (C5H10O5, 150 g mol−1)?

(A) 6.02 × 1022

(B) 6.02 × 1023

(C) 6.02 × 1024

(D) 6.02 × 1025

(E) 6.02 × 1026

184. A compound contains 22.2 percent Ti, 33.3 percent C, and 44.4 percent O. What is the empirical formula for this compound?

(A) TiCO

(B) Ti2C3O4

(C) Ti(CO)2

(D) Ti(CO)3

(E) Ti(CO)6

185. A compound is 92 percent C and 8 percent H. What is the empirical formula for this compound?

(A) CH

(B) CH2

(C) CH4

(D) C6H6

(E) C6H8

186. A compound containing only carbon, hydrogen, and oxygen has a molecular mass of 150 g mol−1. Which of the following may be the empirical formula of the compound?

(A) CHO

(B) C2H3O

(C) CH2O

(D) CH2O2

(E) C5H10O5

187. A compound contains 0.2 mol Pd, 0.8 mol C, 1.2 mol H, and 0.8 mol O. Which of the following is the simplest formula of this compound?

(A) Pd2C8H12O8

(B) Pd2(C4H6O4)2

(C) Pd2(C2H3O2)3

(D) Pd(C2H3O2)3

(E) Pd(C2H3O2)2

188. A compound contains 38 percent F and 62 percent Xe. The empirical formula of the compound is:

(A) XeF

(B) Xe2F

(C) Xe4F

(D) XeF4

(E) Xe2F3

189. What is the empirical formula for a hydrocarbon that is 75 percent carbon by mass?

(A) CH2

(B) CH4

(C) CH6

(D) C4H

(E) C4H5

190. What mass of Cu(s) is produced when 0.050 mol Cu2O (143 g mol−1) is reduced with excess H2(g)?

(A) 3.18 g

(B) 6.35 g

(C) 12.7 g

(D) 31.8 g

(E) 63.5 g

Questions 191–196 refer to the following answer choices:

(A) HCl(aq) + NH3(aq) → NH4Cl(aq) + H2O(l)

(B) Ag+(aq) + Cl(aq) → AgCl(s)

(C) Mg(s) + O2(g) → MgO2(s)

(D) PtCl4(s) + 2 Cl(aq) → PtCl62–(aq)

(E) 3 Cl2(aq) + 6 OH(aq) → 5 Cl(aq) + ClO3(aq) + 3H2O(l)

191. A reaction that produces a coordination complex

192. A reaction in which the same reactant undergoes an oxidation and a reduction

193. A neutralization reaction

194. A precipitation reaction

195. A combustion reaction

196. A reaction that produces an acidic salt

197. All of the following chemical equations represent the correct net ionic equation for the reaction that occurs when aqueous sodium hydroxide is added to a saturated solution of aluminum hydroxide except:

(A) Al(OH)3 + OH → [Al(OH)4]

(B) Al(OH)3 + 3 OH → [Al(OH)6]3–

(C) Al3+ + 4 OH → [Al(OH)4]

(D) Al3+ + 6 OH → [Al(OH)6]3–

(E) Al + 3 OH → Al(OH)3

198. Which of the following chemical equations represents the intense heating of solid hydrogen carbonate (sodium bicarbonate)?

(A) NaHCO3 → Na+ H2O + CO2

(B) NaHCO3 → Na2CO3 + H2O + CO2

(C) NaHCO3 → Na+ H2 + O2 + CO2

(D) Na(CO3)2 → Na + Na2CO3 + H2O + CO2

(E) Na(CO3)2 → Na2CO3 + H2O + CO2

199. Which of the following chemical equations represents the reaction that occurs when pure, solid white phosphorus burns in air?

(A) 4 P + 3 O2 → 2 P4O3

(B) 4 P + 3 O2 → P4O6

(C) 4 P + 5 O2 → P4O10

(D) P4 + 3 O2 → P4O6

(E) P4 + O2 → P4O10

200. Which of the following chemical equations represents the net ionic equation for the reaction that occurs when sodium iodide solution is added to a solution of lead (II) acetate?

(A) 2 I + Pb2+ → PbI2

(B) Na+ + CH3COO → NaCH3COO

(C) 2 NaI + Pb(CH3COO)2 → 2 NaCH3COO + PbI2

(D) 2 NaI + Pb(CH3COO)2 + H2O → 2 NaOH + Pb(OH)2 + I2

(E) 3 I + Pb2+ + 2 H2O → PbI2 + Pb(OH)2 + HI

201. All of the following pairs of substances give visible or tactile (through the production or absorption of a significant amount of heat) evidence of a chemical reaction upon mixing except:

(A) HCl(aq) and KOH(aq)

(B) CaCO3(aq) and HF(aq)

(C) Mg(s) and HI(aq)

(D) Pb(NO3)2(aq) and NaCl(aq)

(E) NH4NO3(aq) and HCl(aq)

Questions 202–205 refer to the following answer choices:

(A) MgO + CO2 → MgCO3

(B) I + Cd2+ → CdI42–

(C) SiH4 + O2 → SiO2 + H2O

(D) CaO + SO2 → CaSO3

(E) Mg(s) → Mg2+ + 2 e

202. A combustion reaction

203. A reaction that produces a complex ion

204. An oxidation that is not a combustion

205. A reaction in which the product forms a gas in acidic solutions

206. When the equation for the reaction of hexane in air is correctly balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2 is:

(A) 6

(B) 12

(C) 14

(D) 19

(E) 25

image

207. When the equation above is balanced and all coefficients reduced to their lowest whole number terms, the coefficient for H2O(l) is:

(A) 7

(B) 6

(C) 5

(D) 3

(E) 2

image

208. When the equation above is balanced and all coefficients reduced to their lowest whole-number terms, the coefficient for H2O(l) is:

(A) 1

(B) 2

(C) 3

(D) 4

(E) 6

image

209. When the equation above is balanced and all coefficients reduced to their lowest whole-number terms, the coefficient for Cl2(g) is:

(A) 2

(B) 3

(C) 4

(D) 5

(E) 6

image

210. When the equation above is balanced and all coefficients reduced to their lowest whole-number terms, the coefficient for H3PO4(l) is:

(A) 1

(B) 2

(C) 3

(D) 4

(E) 5

image

211. The oxidation of ethanol in an acidic solution is represented above. When the equation is balanced and all coefficients reduced to their lowest whole-number terms, the coefficient for H+ is:

(A) 6

(B) 12

(C) 14

(D) 16

(E) 28

image

212. The reaction represented above occurs in a basic solution. When the equation is balanced and all coefficients reduced to their lowest whole-number terms, the coefficient for OH is:

(A) 0

(B) 1

(C) 2

(D) 4

(E) 5

Questions 213–216 refer to the following balanced chemical reaction:

image

213. According to the reaction above, when 0.400 mol of CS2(l) is reacted as completely as possible with 1.20 mol O2(g), the total number of moles of products is:

(A) 0.40

(B) 0.80

(C) 1.20

(D) 1.60

(E) 4.80

214. If 6.30 moles of gas are formed by the reaction indicated above, how many moles of O2(g) are needed to react?

(A) 1.05

(B) 2.10

(C) 4.20

(D) 6.30

(E) 9.45

215. If 33.6 L of product are formed by the above reaction at STP, how many moles of CS2(l) reacted?

(A) 0.50

(B) 1.00

(C) 1.50

(D) 3.00

(E) 3.36

216. An excess of Zn(s) is added to 100 mL of 0.6 M HCl at 0°C and 1 atm. What volume of gas will be produced?

(A) 67.2 mL

(B) 672 mL

(C) 1.3 L

(D) 2.24 L

(E) 6.7 L

Questions 217–219 refer to the following answer choices and the reaction represented below.

image

image

217. The reactants that would produce 3 mol SO3 with one mol O2 in excess

218. Products of the reaction to completion if 4 mol SO2 combine with 1 mol O2

219. Products if 5 mol SO2 reacts with 6.5 mol O2

Questions 220–224 refer to the following chemical reaction:

image

220. If 1.7 g NH3 (17 g mol−1) are mixed with 3.2 g O2 (32 g mol−1), what is the maximum mass of NO (30 g mol−1) that can be produced?

(A) 0.40 g

(B) 2.4 g

(C) 3.2 g

(D) 4.0 g

(E) 4.8 g

221. Suppose NH3 and O2 were mixed in a 4:5 molar ratio. When the reaction was completed, 228 grams of the reaction gases were recovered. Assuming the reaction mixture reacted completely and the gases collected contain 100 percent products, what masses of NO and H2O are expected to be present?

image

222. If 100 mL of distilled water is added to 400 mL of 0.375 M NaCl, which of the following is closest to the Na+ concentration in the final solution?

(A) 0.15 M

(B) 0.19 M

(C) 0.30 M

(D) 0.33 M

(E) 0.69 M

223. How many moles of oxygen gas would be required to produce 1.0 L of NO at STP?

image

224. If 2.5 mol NH3 reacted with 2.5 mol O2 as completely as possible, how many moles of reactant would remain unreacted (in excess)?

(A) 0.50 mol O2

(B) 0.50 mol NH3

(C) 0.63 NH3

(D) 2.0 mol O2

(E) 2.0 mol NH3

Questions 225–227 refer to the following reaction of potassium superoxide (KO2). KO2 is used for its ability to absorb carbon dioxide gas and release oxygen.

image

225. According to the equation above, how many moles of O2(g) can be released if 6.00 mol KO2 and 9.00 mol of CO2(g) are available?

(A) 4.50

(B) 6.00

(C) 9.00

(D) 12.0

(E) 13.5

226. What volume of CO2 is required to react with excess KO2 to produce 6 L of O2(g) at STP?

(A) 4.00 L

(B) 11.2 L

(C) 14.9 L

(D) 22.4 L

(E) 89.6 L

227. When 2.9 g CO2(g) (molar mass 44 g mol−1) reacts with excess KO2 according to the equation above, the volume of O2(g) produced at STP is closest to:

(A) 2.2 L

(B) 4.4 L

(C) 11.2 L

(D) 22.4 L

(E) 33.6 L

228. Which of the following is the correct net ionic equation for the reaction of sodium hydroxide and nitric acid?

(A) H+ + OH → H2O

(B) Na+ + NO3 → NaNO3

(C) NaOH + HNO3 → NaNO3 + H2O

(D) Na+ + OH + H+ + NO3 → NaNO3 + H2O

(E) Na+ + OH + 2 H+ → NaOH + H2

229. Which of the following is an addition reaction?

(A) CH4 + Cl2 → CH3Cl + HCl

(B) CH2=CH2 + Cl2 → CH2ClCH2Cl

(C) C4H10 + Cl2 → C4H10Cl + HCl

(D) CH3(CH2)6CH=CHCOOH + NaOH → CH3(CH2)6CH=CHCOONa + H2O

(E) 6 CO2 + 6 H2O → C6H12O6 + 6 O2

230. Which of the following is a product of the reaction between carbon dioxide and water, CO2(g) + H2O(l)?

I. H+

II. CO32–

III. HCO3

(A) I only

(B) I and II only

(C) I and III only

(D) II and III only

(E) I, II, and III