Consider the following generic equation:

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

2.0 mol A and 1.0 mol B react to form 1.0 mol C. What is the percent yield of this reaction?

Please help! thanks!

You need 3 mol of A for every mol of B

but you only have 2 mol A
so you only use 2/3 of a mol of B
that would yield 4/3 mol of C
but we only got 1 mol of C
100 * 1/(4/3) = 75 % yield

To find the percent yield of a reaction, we need to compare the actual yield to the theoretical yield.

In this case, we are given that 2.0 mol of A and 1.0 mol of B react to form 1.0 mol of C. Let's first determine the theoretical yield, which is the maximum amount of product that could be formed assuming complete conversion and no side reactions.

From the balanced equation, we can see that the stoichiometric ratio between A and C is 3:2. Therefore, if 2.0 mol of A reacts, it would produce (2.0 mol A) x (2 mol C / 3 mol A) = 1.33 mol C. However, we are given that the actual yield of C is 1.0 mol.

Now we can calculate the percent yield using the formula:

Percent Yield = (Actual Yield / Theoretical Yield) x 100

Substituting the values, we get:

Percent Yield = (1.0 mol / 1.33 mol) x 100

Percent Yield ≈ 75.2%

Therefore, the percent yield of this reaction is approximately 75.2%.