How much oxygen is required to completely burn 3.4 grams of hydrogen sulfide?

univerkov | December 5, 2020 | education

Given:
m (H2S) = 3.4 g
V (O2) -?
Explanation:
M (H2S) = 34 g / mol
n (H2S) = m / M = 3.4 g / 34 g / mol = 0.1 mol
2H2S + 3O2 = 2H2O + 2SO2
It can be seen from the UHR that n (O2) = 1.5n (H2S)
n (O2) = 1.5 * 0.1 mol = 0.15 mol
V (O2) = n (O2) * Vm = 0.15 mol * 22.4 L / mol = 3.36 L
Answer 3.36 L

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