Question

Hydrogen sulfide gas reacts with oxygen to produce sulfur dioxide gas and water according to the balance equation:

2H2S + 3O2 → 2SO2 + 2H2O.
How many moles of oxygen gas are required to react with 5.6 moles of hydrogen sulfide?

Answer 1

To react with 5.6 moles of hydrogen sulfide, 8.4 moles of oxygen gas are required.

Step-by-step explanation:

The balanced equation for the reaction between hydrogen sulfide and oxygen is: 2H2S + 3O2 → 2SO2 + 2H2O

To find out how many moles of oxygen gas are required to react with 5.6 moles of hydrogen sulfide, we can use the stoichiometric coefficients from the balanced equation.

From the balanced equation, we can see that the ratio of moles of hydrogen sulfide to moles of oxygen gas is 2:3. Therefore, for every 2 moles of hydrogen sulfide, we need 3 moles of oxygen gas.

Therefore, to react with 5.6 moles of hydrogen sulfide, we would need:

(5.6 moles H2S) * (3 moles O2) / (2 moles H2S) = 8.4 moles of oxygen gas

Answer 2

2 mol of H2S react with 3 mol of O2

5.6 mol of H2S react with =5.6×3/2=8.4 mol of O2