What is the percentage yield for a reaction if you predict the formation of 21 grams of C6H12 and actually recomvered only 3.8 grams?

is the answer 18%
3.8g/21g x 100%
pls verify.

Yes, correct.

Well, let me do the math here.

The formula for calculating percentage yield is (actual yield / predicted yield) x 100.

So, if you recovered 3.8 grams and predicted the formation of 21 grams, the calculation would be:

(3.8g / 21g) x 100% = 18.0952381%

But hey, let's not get too caught up in the decimals. We can round it off to 18% for simplicity's sake. So yes, your answer is correct, my friend! 18% it is!

To calculate the percentage yield of a reaction, you need to divide the actual yield by the theoretical yield, and then multiply by 100 to get the percentage.

In this case, the predicted formation of C6H12 is 21 grams, and the actual recovered amount is 3.8 grams.

The percentage yield can be calculated as follows:

(3.8 g / 21 g) x 100% = 18.1%

So, the correct answer is 18.1%, which means the actual yield is 18.1% of the predicted yield.

To calculate the percentage yield of a reaction, you divide the actual yield by the theoretical yield and multiply it by 100%.

Theoretical yield refers to the maximum amount of product that can be obtained based on stoichiometry and initial reactant amounts. In this case, the theoretical yield is 21 grams of C6H12.

Actual yield refers to the amount of product that is actually obtained from the reaction. In this case, the actual yield is 3.8 grams of C6H12.

So, in order to calculate the percentage yield, you need to divide the actual yield by the theoretical yield and multiply by 100%:

Percentage yield = (Actual yield / Theoretical yield) x 100%

Let's substitute the values:

Percentage yield = (3.8g / 21g) x 100% = 0.18 x 100% = 18%

So, your calculation is correct. The percentage yield for the reaction is indeed 18%.