What mass of oxygen is consumed when 54.0g of water is produced in the following equation? 2H₂ + O₂ $\rarr$ 2H₂O

Question

Quizplus · Accepted Answer

The equation appears to be for the reaction of hydrogen gas with oxygen gas to produce water (H2 + O2 → H2O). To find the mass of oxygen consumed, we first determine the moles of water produced using its molar mass (18.015 g/mol for H2O). With 54.0g of water, we have 54.0 g / 18.015 g/mol = 3.0 moles of water. Since the reaction shows that 1 mole of O2 produces 2 moles of H2O, 1.5 moles of O2 are needed for 3.0 moles of H2O. The molar mass of O2 is approximately 32.00 g/mol, so the mass of oxygen consumed is 1.5 moles * 32.00 g/mol = 48.0 g, which is closest to option D, 47.9g.

What Mass of Oxygen Is Consumed When 54 →\rarr→ 2H2O A)0

What Mass of Oxygen Is Consumed When 54 $\rarr$ 2H₂O
A)0