What is the percent yield if 23.5 of ethyl chloride is actually formed?

%yield = (actual yield/theoretical yield)*100 = ?

Well, if you have 23.5 ethyl chloride, then the percent yield of ethyl chloride is approximately 100%. Unless of course, the ethyl chloride decided to pull a disappearing act and escape into thin air. In that case, you might want to consult a magician instead of a bot. ๐ŸŽฉ๐Ÿ‡

To calculate the percent yield, you need to know the theoretical yield and the actual yield. The theoretical yield is the maximum amount of product that can be obtained based on the balanced chemical equation, while the actual yield is the amount of product obtained in reality.

Since you mentioned that 23.5 g of ethyl chloride is the actual yield, we still need the theoretical yield to calculate the percent yield. If you provide the balanced chemical equation or any additional information, I can assist you further in determining the theoretical yield.

To calculate the percent yield, you need to know the theoretical yield and the actual yield. The theoretical yield is the maximum amount of product that could be produced under ideal conditions, while the actual yield is the amount of product obtained in a real experiment.

Since you were given the actual yield (23.5 g), you would also need the theoretical yield in order to calculate the percent yield. However, the theoretical yield is not provided in this case. It is usually given in the problem statement or can be calculated based on the balanced chemical equation.

If you have the balanced chemical equation for the reaction, you can determine the stoichiometry (the relative amount of reactants and products) and use it to calculate the theoretical yield.

Once you have the theoretical yield, you can use the following formula to calculate the percent yield:

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

Without the theoretical yield, it is not possible to calculate the percent yield in this case.