Question

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 CO_{2 (g)} + 4 H_{2 (g)} → HC₂H₃O_{2 (g)} + 2 H₂O _(g)

Use the correct number of significant figures.

Answer 1

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