A reaction was performed in which 3.6 g 3.6 g of benzoic acid was reacted with excess methanol to make 1.3 g 1.3 g of methyl benzoate. Calculate the theoretical yield and percent yield for this reaction.

The percent yield of the reaction is 32.34 %

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of benzoic acid = 3.6 g

Molar mass of benzoic acid = 122.12 g/mol

Putting values in equation 1, we get:

The chemical equation for the reaction of benzoic acid and methanol is:

By Stoichiometry of the reaction

1 mole of benzoic acid produces 1 mole of methyl benzoate

So, 0.0295 moles of benzoic acid will produce = moles of methyl benzoate

Molar mass of methyl benzoate = 136.15 g/mol

Moles of methyl benzoate = 0.0295 moles

Putting values in equation 1, we get:

Experimental yield of methyl benzoate = 1.3 g

Theoretical yield of methyl benzoate = 4.02 g

Putting values in above equation, we get:

Hence, the percent yield of the reaction is 32.34 %

if you mean hydrogen and oxygen then water is the product