Question

3 A+B 2C+D

What is the percent yield of the reaction if 7.00 mol of A actually formed 1.00 mol of
C?

Answer 1

Percent Yield = 21.4% C

Step-by-step explanation:

The actual yield is the value that was produced after conducting an experiment. The theoretical yield is the value calculated using the balanced chemical equation.

To find the percent yield, you need to (1) convert moles A to moles C (via the mole-to-mole ratio from equation coefficients) and then (2) calculate the percent yield. It is important to arrange the ratios in a way that allows for the cancellation of units. The final answer should have 3 sig figs to match the sig figs of the values given.

3 A + B -----> 2 C + D
^ ^

7.00 moles A 2 moles C
--------------------- x ---------------------- = 4.67 moles C
3 moles A

Actual Yield
Percent Yield = ------------------------------ x 100%
Theoretical Yield

1.00 moles C
Percent Yield = ------------------------- x 100%
4.67 moles C

Percent Yield = 21.4% C