You are given the balanced chemical equation:
C₄H₄ + 5 O₂ $\rarr$ 4 CO₂ + 2 H₂O If 0.3618 moles of C₄H₄ are allowed to react with 1.818 moles of O₂, and this is the only reaction which occurs, what is the maximum mass of water that could be produced?

Question

You are given the balanced chemical equation:
C₄H₄ + 5 O₂

\rarr

4 CO₂ + 2 H₂O If 0.3618 moles of C₄H₄ are allowed to react with 1.818 moles of O₂, and this is the only reaction which occurs, what is the maximum mass of water that could be produced?

Quizplus · Accepted Answer

The limiting reactant is O₂, as 1.818 moles is less than the 1.809 moles required to fully react with 0.3618 moles of C₄H₄. From the balanced equation, 5 moles of O₂ produce 2 moles of H₂O. Thus, 1.818 moles of O₂ produce (1.818/5)*2 = 0.7272 moles of H₂O. The molar mass of H₂O is 18.02 g/mol, so the mass of water produced is 0.7272 moles * 18.02 g/mol = 13.104 g, which rounds to 13.04 g.

You Are Given the Balanced Chemical Equation: C4H4 + 5 →\rarr→

You Are Given the Balanced Chemical Equation:
C₄H₄ + 5 $\rarr$