Question

1. The combustion of 0.136 kg of methane in the presence of excess oxygen produces 353 g of carbon dioxide. What is the percent yield?

A. 94.6 %
B. 38.5 %
C. 0.946 %

2. The combustion of 8.0 g of methane in the presence of excess oxygen produces 19.5 g of carbon dioxide. What is the limiting reactant?

A. carbon dioxide
B. methane
C. oxygen

3. The combustion of 0.1240 kg of propane in the presence of excess oxygen produces 0.3110 kg of carbon dioxide. What is the theoretical yield?

A. 371.2 g
B. 0.3712 g
C. 0.8377 g

Please explain steps. Thank you!

Answer 1

you know its a combustion reaction, and a combustion reaction always has the same general "look" \[fuel + O_2 \rightarrow CO_2 + H_2O\] each fuel is slightly different, but they all contain carbons and hydrogens.

You need to write a balanced reaction, then use the mass of each fuel they give you to find the \(theoretical\) yield of carbon dioxide, then compare that to the actual yield they give you to find the percent yield