9.Nickel, a common metal used in a variety of alloys, is purified via the Mond process to a very high (> 99.99%) purity. One of the steps in the Mond process involves the reaction of solid nickel with carbon monoxide to produce Ni(CO)4, as shown in the unbalanced equation below.
Ni(s) + CO(g) â Ni(CO)4(g)
How much carbon monoxide, in grams, is required to purify an impure sample containing 3.82 kg of nickel?
10.Thermite is a metal powder mixture used frequently in pyrotechnics and metal construction work. It is composed of highly powderized aluminum and iron(III) oxide and when ignited by a high temperature source (such as burning magnesium ribbon), it reacts according to the following equation.
Fe2O3(s) + 2 Al(s) â 2 Fe(l) + Al2O3(s)
What mass of powderized Al is required to completely react with 34.8 g Fe2O3?
11.In a reaction vessel, 18.0 g of solid chromium(III) oxide, Cr2O3, was allowed to react with excess carbon tetrachloride in the following reaction.
Cr2O3(s) + 3 CCl4(l) â 2 CrCl3(s) + 3 COCl2(aq)
Determine the percent yield of the reaction, given that the actual yield of chromium chloride, CrCl3, was 29.5 g. (The molar mass of Cr2O3 is 152.00 g/mol and the molar mass of CrCl3 is 158.35 g/mol.)
12. Ammonia (NH3) can be synthesized from nitrogen gas (N2) and hydrogen gas (H2) by the following reaction.
N2(g) + 3 H2(g) â 2 NH3(g)
If the theoretical yield of ammonia is 327 g and the actual yield is 237 g, calculate the percent yield of ammonia.
13.In making wine, glucose (C6H12O6) is fermented to produce ethanol (C2H5OH) and carbon dioxide (CO2), according to the following reaction.
C6H12O6 â 2 C2H5OH + 2 CO2
(a) If the fermentation reaction starts with 62.0 g glucose, what is the theoretical yield of ethanol (in grams)?
b.If 12.0 g ethanol is produced, what is the percent yield of this reaction?
9.Nickel, a common metal used in a variety of alloys, is purified via the Mond process to a very high (> 99.99%) purity. One of the steps in the Mond process involves the reaction of solid nickel with carbon monoxide to produce Ni(CO)4, as shown in the unbalanced equation below.
Ni(s) + CO(g) â Ni(CO)4(g)
How much carbon monoxide, in grams, is required to purify an impure sample containing 3.82 kg of nickel?
10.Thermite is a metal powder mixture used frequently in pyrotechnics and metal construction work. It is composed of highly powderized aluminum and iron(III) oxide and when ignited by a high temperature source (such as burning magnesium ribbon), it reacts according to the following equation.
Fe2O3(s) + 2 Al(s) â 2 Fe(l) + Al2O3(s)
What mass of powderized Al is required to completely react with 34.8 g Fe2O3?
11.In a reaction vessel, 18.0 g of solid chromium(III) oxide, Cr2O3, was allowed to react with excess carbon tetrachloride in the following reaction.
Cr2O3(s) + 3 CCl4(l) â 2 CrCl3(s) + 3 COCl2(aq)
Determine the percent yield of the reaction, given that the actual yield of chromium chloride, CrCl3, was 29.5 g. (The molar mass of Cr2O3 is 152.00 g/mol and the molar mass of CrCl3 is 158.35 g/mol.)
12. Ammonia (NH3) can be synthesized from nitrogen gas (N2) and hydrogen gas (H2) by the following reaction.
N2(g) + 3 H2(g) â 2 NH3(g)
If the theoretical yield of ammonia is 327 g and the actual yield is 237 g, calculate the percent yield of ammonia.
13.In making wine, glucose (C6H12O6) is fermented to produce ethanol (C2H5OH) and carbon dioxide (CO2), according to the following reaction.
C6H12O6 â 2 C2H5OH + 2 CO2
(a) If the fermentation reaction starts with 62.0 g glucose, what is the theoretical yield of ethanol (in grams)?
b.If 12.0 g ethanol is produced, what is the percent yield of this reaction?
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