The amount of carbon dioxide evolved upon complete combustion of 116 g of n -butane is (Given: atomic mass in amu H =1 , C =12 and O =16 )

Step-by-step solution

The balanced chemical equation for the combustion of n -butane is: C₄H₁₀ + 13 2 O₂ 4CO₂ + 5H₂O Molar mass of n -butane ( C₄H₁₀ ) = 4 12 + 10 1 = 58 g/mol Number of moles of n -butane = 116 58 = 2 moles From the balanced equation, 1 mole of n -butane produces 4 moles of CO₂ . Number of moles of CO₂ produced = 2 4 = 8 moles Molar mass of CO₂ = 12 + 2 16 = 44 g/mol Mass of CO₂ produced = 8 44 = 352 g Answer: 352 g