Question

If a reaction has a theoretical yield of 53.55 g and had a 78.5 % yield, then what was the actual yield isolated for that reaction?

Answer 1

Answer:

So, you know that your reaction has a theoretical yield of

82.5 g

. This means that if all the moles of reactants that take part in the reaction end up producing moles of product according to the reaction's stoichiometric coefficients, you will get

82.5 g

of product.

In other words, the theoretical yield tells you how much product is produced for a

100

%

yield.

Now, the reaction is said to produce

12.3 g

less than expected. This means that you only collected

actual yield

=

82.5 g

−

12.3 g

=

70.2 g

The reaction's percent yield will thus be

% yield

=

70.2

g

82.5

g

×

100

=

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

85.1%

a

a

∣

∣

−−−−−−−−−−

The answer is rounded to three sig figs.