Electrolysis of 12.6 g of water would produce what volume of O₂ gas at 640 torr and
22) 0 °C?
2 H₂O (l) + electricity $\rightarrow$ 2 H₂(g) + O₂(g)

Question

Electrolysis of 12.6 g of water would produce what volume of O₂ gas at 640 torr and 22)0 °C? 2 H₂O (l) + electricity $\rightarrow$ 2 H₂(g) + O₂(g)

Quizplus · Accepted Answer

The molar mass of water (H₂O) is 18 g/mol. Therefore, 12.6 g of water is 12.6 g / 18 g/mol = 0.7 mol. According to the balanced equation, 2 moles of water produce 1 mole of O₂. Thus, 0.7 mol of water will produce 0.35 mol of O₂. Using the ideal gas law and converting the pressure to atm (640 torr = 0.842 atm) and temperature to Kelvin (22°C = 295 K), the volume V = nRT/P = (0.35 mol)(0.0821 L·atm/mol·K)(295 K) / 0.842 atm = 10.1 L.

Electrolysis of 12 →\rightarrow→ 2 H2(g) + O2(g) A) 10

Electrolysis of 12 $\rightarrow$ 2 H₂(g) + O₂(g)
A) 10