Question

Determine the theoretical maximum moles of hydroquinone, , that could be produced in this experiment. The reactant, quinone, is the limiting reagent. (To avoid introducing rounding errors on intermediate calculations, enter your answer to four significant figures.)


Reactant mass 23.4g
Product mass 13.0g
Reactant moles 0.2167 mol

Reactant mass 23.4g
Product mass 13.0g
Molar mass C 12.0 g/mol
Molar mass H 1.00 g/mol
Molar mass O 16.0 g/mol

Theoretical maximum moles of hydroquinone:___________

Answer 1

Answer:

Theoretical maximum moles of hydroquinone: 0.2167 mol.

Explanation:

Hello,

In this case, the undergoing chemical reaction is like:

$Quinone\rightarrow Hydroquinone$

In such a way, since the molar mass of quinone is 108.1 g/mol and it is in a 1:1 molar ratio with hydroquinone, we can easily compute the theoretical maximum moles of hydroquinone by stoichiometry:

$n_{hydroquinone}=23.4g\ quinone*\frac{1mol\ quinone}{108.1 g\ quinone}*\frac{1mol\ hydroquinone}{1mol\ quinone} \\\\n_{hydroquinone}=0.2167mol$

Clearly, this is the theoretical yield which in grams is:

$m_{hydroquinone}=0.2167mol*\frac{110.11g}{1mol} =23.84g$

Which allows us to compute the percent yield as well since the obtained mass of the product is 13.0 g:

$Y=\frac{13.0g}{23.84g}*100\%=54.5\%$

Best regards.