Question

Consider the balanced chemical

reaction below. When the reaction was
carried out, the calculated theoretical
yield for iron was 365 grams, but the
measured yield was 278 grams. What
is the percent yield?
Fe2O3 + 3C0 2Fe + 3C02

Answer 1

Step-by-step explanation:

Percentage yield = (278/365) * 100% = 76.16%.

Answer 2

`\boxed {\boxed {\sf 76.2 \% }}`

Step-by-step explanation:

A percent yield helps measure how successful or precise a reaction was. It is ratio of measured yield to theoretical yield as a percent. The formula is:

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

For this reaction, the measured/actual yield was 278 grams, while the theoretical yield was 365 grams.

`actual = 278 \ g \\\theoretical= 365 \ g`

Substitute the values into the formula.

`percent \ yield =(278 \ g)/(365 \ g) *100`

Divide first. The grams (g) will cancel out.

• 278 g/365 g= 278/365=0.7616438356

`percent \ yield =0.76164383561*100`

Multiply.

`percent \ yield=76.1643835616`

The original measurements both had 3 significant figures, so we should round our percent yield to 3 sig figs. In this case, that is the tenths place.

The 6 in the tenth place tells us to round the 1 up to a 2.

`percent \ yield \approx 76.2`

The percent yield is about 76.2 %