Chapter 03 – Mass Relationships in Chemical Reactions
165. Balance the following chemical equation: C3H6O + O2 → CO2 + H2O
166. Balance the following chemical equation:
C + Fe2O3 → Fe + CO
Chapter 03 – Mass Relationships in Chemical Reactions
167. Balance the following chemical equation:
P4O10 + H2O → H3PO4
168. Balance the following chemical equation:
Al(s) + Co(NO3)2(aq) → Al(NO3)3(aq) + Co(s)
Chapter 03 – Mass Relationships in Chemical Reactions
169. Refer to the (unbalanced) equation CS2 + CaO → CO2 + CaS. How many grams of CaS
170. Refer to the (unbalanced) equation CS2 + CaO → CO2 + CaS. How many grams of CaO
are required to react completely with 38 g of CS2?
Chapter 03 – Mass Relationships in Chemical Reactions
171. How many grams of silver nitrate are necessary to react completely with 7.000 moles of
copper?
Cu + 2 AgNO3 → Cu(NO3 )2 + 2 Ag
172. What mass of sodium nitrate would be produced from the complete reaction of 1.00 mol
of lead nitrate?
2 NaCl + Pb(NO3 )2 → 2 NaNO3 + PbCl2
Chapter 03 – Mass Relationships in Chemical Reactions
173. What is the minimum mass of sulfur dioxide necessary to produce 200. g of sulfuric acid
in the following reaction?
2SO2 + O2 + 2H2O → 2H2SO4
174. What is the minimum mass of oxygen gas necessary to produce 200. g of sulfuric acid in
the following reaction?
2SO2 + O2 + 2 H2O → 2H2SO4
Chapter 03 – Mass Relationships in Chemical Reactions
175. What is the minimum mass of water necessary to produce 200. g of sulfuric acid in the
following reaction?
2SO2 + O2 + 2H2O → 2H2SO4
176.
How many moles of phosphine (PH3) are produced for every 4.0 moles of hydrogen that react according to the chemical
equation below?
3H2 + P2 → 2PH3
Chapter 03 – Mass Relationships in Chemical Reactions
177. Calculate the mass of sodium chlorate that must decompose to form 6.5 g of oxygen.
2NaClO3(s) → 2NaCl(s) + 3O2(g)
178. What is the theoretical yield of PI3 if 48.0 g of I2 are reacted with an excess of
phosphorus according to the following chemical equation?
2P(s) + 3I2(s) → 2PI3(s)
Chapter 03 – Mass Relationships in Chemical Reactions
179. Phosphorus reacts with iodine as shown in the chemical reaction below. What is the
percent yield of the reaction if 28.2 g PI3 is obtained from the reaction of 48.0 g of I2 with
excess phosphorus?
2P(s) + 3I2(s) → 2PI3(s)
180. What is the limiting reagent when 27.0 g of P and 68.0 g of I2 react according to the
following chemical equation?
2P(s) + 3I2(s) → 2PI3(s)
Chapter 03 – Mass Relationships in Chemical Reactions
181. Determine the number of moles of water produced by the reaction of 155 g of ammonia
and 356 g of oxygen.
4NH3 + 5O2 → 4NO + 6H2O
182. What is the theoretical yield of PI3 from the reaction of 27.0 g of P and 68.0 g of I2?
2P(s) + 3I2(s) → 2PI3(s)
Chapter 03 – Mass Relationships in Chemical Reactions
183. When a 0.860 g sample of an organic compound containing C, H, and O was burned
completely in oxygen, 1.64 g of CO2 and 1.01 g of H2O were produced. What is the empirical
formula of the compound?
184. When a 0.952 g sample of an organic compound containing C, H, and O is burned
completely in oxygen, 1.35 g of CO2 and 0.826 g of H2O are produced. What is the empirical
formula of the compound?
Chapter 03 – Mass Relationships in Chemical Reactions
185. The percent composition by mass of tartaric acid is: 32.01% C, 4.03% H, and 63.96% O.
186. Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen.
The product that was purified and sent off for elemental analysis giving the following mass
percents: 68.85% C and 4.95% H. Determine the empirical formula of this compound.
Chapter 03 – Mass Relationships in Chemical Reactions
187. Pressurized metal gas cylinders are generally used to store commonly used gases in the
laboratory. At times it can be easier to chemically prepare occasionally used gases. For
example, nitrogen monoxide, NO(g), can be prepared in the lab using the following chemical
reaction:
3Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l)
If 5.0 g of copper metal was added to an aqueous solution containing 2.5 moles of HNO3, how
many moles of NO(g) would be produced, assuming a 100% yield?
188. Pressurized metal gas cylinders are generally used to store commonly used gases in the
laboratory. At times, it can be easier to chemically prepare occasionally used gases. For
example, nitrogen monoxide, NO(g), can be prepared in the lab by the following chemical
reaction:
3Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l)
If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO3, how
many moles of NO(g) would be produced, assuming a 75% yield?
Chapter 03 – Mass Relationships in Chemical Reactions
189. Pressurized metal gas cylinders are generally used to store commonly used gases in the
laboratory. At times, it can be easier to chemically prepare occasionally used gases. For
example, oxygen gas can be prepared by heating KMnO4(s) according to the following
chemical reaction:
2KMnO4(s) → K2MnO4(s) + MnO2(s) + O2(g)
How many grams of KMnO4 would you need to produce 0.27 moles of O2, assuming 100%
190. Pressurized metal gas cylinders are generally used to store commonly used gases in the
laboratory. At times, it can be easier to chemically prepare occasionally used gases. For
example, oxygen gas can be prepared by heating KMnO4(s) according to the following
chemical reaction:
2KMnO4(s) → K2MnO4(s) + MnO2(s) + O2(g)
The above procedure was carried out starting with 93.2 g of KMnO4, and it was later
determined that all of the KMnO4 reacted according to the above equation except 11.7 g.
What was the percent yield for the reaction?
Chapter 03 – Mass Relationships in Chemical Reactions
191. In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia. How
many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen,
and how many kilograms of ammonia would be formed?
192. Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the
following reaction:
NH4NO3 → N2O + 2H2O
If a 108 g sample of NH4NO3 decomposes to give 23 g of N2O(g), what percent of the original
sample remains?
Chapter 03 – Mass Relationships in Chemical Reactions
193. Ferrocene, Fe(C5H5)2(s), can be prepared by reacting 3.0 g of FeCl2(s) with an equal
mass of cyclopentadiene, C5H6(l), and an excess of KOH, as shown in the following reaction
FeCl2 + 2C5H6 + 2KOH → FeC10H10 + 2H2O
A student who carried out this reaction obtained 2.7 g of ferrocene. Of the following choices
which has three correct answers?
194. Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide
to excess water, as shown in the following reaction
CaC2(s) + H2O(l) → HCCH(g) + CaO(s)
How many grams of CaC2 would be required to generate 0.20 moles of HCCH(g)?