How much hydrogen is required for the reaction with a sulfur mass of 9.6 g?

Given:

m (S) = 9.6 g;

To find:

V (H2) -?

Decision:

1) H2 + S – (load) -> H2S, – we solve the problem using the composed reaction equation.

2) Find the amount of sulfur contained in 9.6 grams of the substance:

n (S) = m: M = 9.6 g: 32 g / mol = 0.3 mol;

3) We compose logical equality:

if 1 mole of S requires 1 mole of H2,

then 0.3 mol S will require x mol H2,

then x = 0.3 mol.

4) Find the volume of hydrogen required for the reaction to proceed:

V (H2) = n * Vm = 0.3 mol * 22.4 L / mol = 6.72 L.

Answer: V (H2) = 6.72 liters.