Technical Na with a mass of 50 g reacts with h2o and a gas with a volume of 22.4 liters
Technical Na with a mass of 50 g reacts with h2o and a gas with a volume of 22.4 liters is released. Find the mass fraction of impurities in Na.
Let’s write the reaction equation:
2Na + 2H2O = 2NaOH + H2 ↑
Let’s find the amount of substance of the released hydrogen gas:
v (H2) = V (H2) / Vm = 22.4 / 22.4 = 1 (mol).
According to the reaction equation, 1 mol of H2 is formed from 2 mol of Na, therefore:
v (Na) = v (H2) * 2 = 1 * 2 = 2 (mol).
Let’s find the mass of pure sodium in a sample of technical sodium:
m (Na) = v (Na) * M (Na) = 2 * 23 = 46 (g).
Let’s find the mass of impurities in a sample of technical sodium:
m (impurities) = m (Na) tech. – m (Na) = 50 – 46 = 4 (g).
Let’s find the mass fraction of impurities in a sample of technical sodium:
w (impurities) = (m (impurities) / m (Na) tech.) * 100 = (4/50) * 100 = 8 (%).
Answer: 8%.