How many liters of hydrogen gas are needed to produce 90.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below?
2 H₂(g) + O₂(g) → 2 H₂O(l)

Question

Quizplus · Accepted Answer

To find the volume of hydrogen gas needed, first calculate the moles of water produced: 90.0 g H2O / 18.015 g/mol = 5.0 mol H2O. According to the balanced equation, 2 moles of H2 produce 2 moles of H2O, so 5.0 mol H2O requires 5.0 mol H2. Using the ideal gas law (PV=nRT), where R=0.0821 L·atm/mol·K and T=298 K (25°C), the volume V = nRT/P = (5.0 mol)(0.0821 L·atm/mol·K)(298 K) / (1.00 atm) = 122 L.

How Many Liters of Hydrogen Gas Are Needed to Produce