How many grams of water are produced by burning 7.0 g of C₂H₄ in excess O₂?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the combustion of C₂H₄ is: C₂H₄ + 11O2 → 12CO2 + 6H2O + 2SO2 From the equation, we can see that for every mole of C₂H₄ burned, we get 6 moles of water produced. The molar mass of C₂H₄ is 278 g/mol. Therefore, the number of moles of C₂H₄ burned is: 7.0 g / 278 g/mol = 0.0251 mol The number of moles of water produced is: 0.0251 mol x 6 = 0.1506 mol The molar mass of water is 18 g/mol. Therefore, the mass of water produced is: 0.1506 mol x 18 g/mol = 2.71 g, which is closest to answer choice B (9.0 g).

How Many Grams of Water Are Produced by Burning 7