Acetylene (C₂H₂) burns in pure oxygen with a very hot flame. The products of this reaction are carbon dioxide and water. How much oxygen is required to react with 52.0 g of acetylene?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the combustion of acetylene is:C2H2 + 5O2 → 2CO2 + H2OFrom the balanced equation, we can see that 1 mole of acetylene reacts with 5 moles of oxygen. The molar mass of acetylene is 26.04 g/mol, so 52.0 g of acetylene is equal to 2.00 mol. Therefore, the amount of oxygen required to react with 52.0 g of acetylene is 5 x 2.00 mol = 10.0 mol. The molar mass of oxygen is 32.00 g/mol, so 10.0 mol of oxygen is equal to 10.0 mol x 32.00 g/mol = 320.0 g.

Acetylene (C2H2) Burns in Pure Oxygen with a Very Hot

Acetylene (C₂H₂) Burns in Pure Oxygen with a Very Hot