What volume of hydrogen can be obtained by reacting 0.5 g of sodium with water if the product

What volume of hydrogen can be obtained by reacting 0.5 g of sodium with water if the product yield is 96% of the theoretically possible?

Let’s execute the solution:
1. Let’s compose an equation, select the coefficients:
2Na + 2H2O = 2NaOH + H2 – redox reaction, hydrogen is released;
2. Let’s make calculations using the formulas:
M (Na) = 22.9 g / mol;
M (H2) = 2 g / mol.
3. Let’s calculate the amount of sodium moles, if the mass is known:
Y (Na) = m / M = 0.5 / 22.9 = 0.02 mol.
4. Let’s make the proportion:
0.02 mol (Na) – X mol (H2);
-2 mol – 1 mol from here, X mol (H2) = 0.02 * 1/2 = 0.01 mol.
5. Determine the theoretical volume of hydrogen:
1 mol of gas at n. y – 22.4 liters.
0.01 mol – X l. hence, X l (H2) = 0.01 * 22.4 / 1 = 0.224 l.
6. Find the practical volume of hydrogen if the product yield is 96%
0.96 = V (practical) / V (theoretical);
V (practical) = 0.96 * 0.224 = 0.215 liters.
Answer: the volume of hydrogen is 0.215 liters.