In the reaction
2A + B → 3C + D
3.0 mol A and 2.0 mol B react to form 4.0 mol C. What is the percent yield of this reaction?

Question

Quizplus · Accepted Answer

To find the percent yield, first calculate the theoretical yield based on the given amounts of reactants:

- According to the balanced equation, every 2 mol A reacts with 1 mol B to produce 3 mol C. 
- So, with 3.0 mol A and 2.0 mol B, the limiting reactant is B (since there is not enough B to react with all of the A). 
- Therefore, the theoretical yield of C would be (3.0 mol A) x (3 mol C/2 mol A) = 4.5 mol C.

Now, to calculate the percent yield:

- actual yield = 4.0 mol C (given) 
- percent yield = (actual yield/theoretical yield) x 100% = (4.0 mol C/4.5 mol C) x 100% = 88.9%

Rounded to the nearest whole number, the percent yield is 89%. Therefore, the best choice is B.

In the Reaction 2A + B → 3C + D