Question

If 7.0 mol of NO and 5.0 mol of O2 are reacted tegethor. The reaction generates 3.0 mol of NO2. What is the percent yield for the reaction? 2NO(g) + O2(g) -> 2NO2(g)

Answer 1

The percent yield for the reaction is calculated by comparing the actual yield to the theoretical yield, and then multiplying by 100. In this case, the percent yield is 150%.

Step-by-step explanation:

The percent yield for a reaction is calculated by comparing the actual yield to the theoretical yield, and then multiplying by 100. The actual yield is the amount of product obtained from the reaction, which in this case is 3.0 mol of NO2. The theoretical yield is the amount of product that would be obtained if the reaction went to completion, which can be determined by stoichiometry.

From the balanced equation, we can see that the stoichiometric ratio between NO and NO2 is 2:2 (or 1:1). Therefore, for every 2 mol of NO reacted, 2 mol of NO2 are produced. Since the reaction gave 3.0 mol of NO2, it means that 3.0 mol of NO were reacted as well.

Now, let's calculate the theoretical yield:

1. Convert the amount of NO to moles: 7.0 mol - 3.0 mol = 4.0 mol of NO.
2. Using the stoichiometric ratio, for every 2 mol of NO, 2 mol of NO2 are produced. Therefore, the theoretical yield of NO2 is 2.0 mol.
3. Calculate the percent yield: (actual yield / theoretical yield) x 100 = (3.0 mol / 2.0 mol) x 100 = 150%.

Therefore, the percent yield for the reaction is 150%.