Question

Part A

If the theoretical yield of a reaction is 23.5 g and the actual yield is 14.8 g, what is the percent yield?

Answer 1

`\boxed {\boxed {\sf 63.0 \%}}`

Step-by-step explanation:

The percent yield is the ratio of the actual yield to the theoretical yield.

`percent \ yield = (actual \ yield)/(theoretical \ yield) * 100`

• The actual yield is the amount obtained from performing a chemical reaction. For this problem, it is 14.8 grams.
• The theoretical yield is the potential amount from performing a chemical reaction at maximum performance. For this problem, it is 23.5 grams.

We can substitute the known values into the formula.

`percent \ yield= ( 14.8 \ g)/(23.5 \ g)*100`

Divide.

`percent \ yield = 0.629787234043*100`

Multiply.

`percent \ yield = 62.9787234043`

The original measurements for the theoretical and actual yields have 3 significant figures, so our answer must have the same. For the number we calculated, that is the tenths place.

The 7 to the right, in the hundredths place, tells us to round the 9 up to a 0. Since we rounded up to 0, we have to move to the next place to the left and round the 2 up to a 3.

`percent \ yield \approx 63.0`

The percent yield is approximately 63.0 percent.