Question

# What is the theoretical yield (in grams) of acetic acid, HC2H3O2, when 8.925 g of carbon...

 What is the theoretical yield (in grams) of acetic acid, HC2H3O2, when 8.925 g of carbon dioxide reacts with 1.735 g of hydrogen according to the following reaction: 2 CO2 (g) + 4 H2 (g) → HC2H3O2 (g) + 2 H2O (g) Use the correct number of significant figures.

First calculate limiting reagent

molar mass of CO2 = 44.01 gm/mole then 2 mole of CO2 = 88.02 gm

molar mass of H2 = 2.01 gm/mole then 4 mole of H2 = 8.04 gm

According to reaction 2 mole of CO2 react with 4 mole of H2 that mean 88.02 gm of CO2 react with 8.04 gm of H2 then to react with 8.925 gm of CO2 required H2 = 8.04 8.925 / 88.02 = 0.815 gm

but H2 given 1.735 gm therefore H2 is excess reagent and CO2 is limiting reagent react completly.

molar mass of acetic acid = 60.05 gm/mol

According to reaction 2 mole of CO2 produce 1 mole of acetic acid that mean 88.02 gm of CO2 produce 60.05 gm of acetic acid then 8.925 gm of CO2 produce = 60.05 8.925 / 88.02 = 6.0889 gm of acetic acid

theoretical yield of acetic acid = 6.0889 gm

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