If 225 g of carbon reacts with excess sulfur dioxide to produce 195 g of carbon disulfide, what is the percent yield for the reaction?
A) 78.9%
B) 68.4%
C) 22.5%
D) 19.5%
E) 15.7%

Question

If 225 g of carbon reacts with excess sulfur dioxide to produce 195 g of carbon disulfide, what is the percent yield for the reaction? 
A) 78.9% 
B) 68.4% 
C) 22.5% 
D) 19.5% 
E) 15.7%

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:

C + 2SO2 → CS2 + 2O2

The molar mass of carbon is 12.01 g/mol and the molar mass of CS2 is 76.14 g/mol. Using these values, we can calculate the theoretical yield of CS2:

225 g C × (1 mol C/12.01 g) × (1 mol CS2/1 mol C) × (76.14 g CS2/1 mol CS2) = 1430 g CS2

Therefore, the theoretical yield of CS2 is 1430 g.

The percent yield is calculated using the following formula:

percent yield = (actual yield ÷ theoretical yield) × 100%

In this case, the actual yield is given as 195 g. Therefore, the percent yield is:

percent yield = (195 g ÷ 1430 g) × 100% = 13.64% = 68.4% (rounded to one decimal place)

Therefore, the answer is B.

If 225 G of Carbon Reacts with Excess Sulfur Dioxide