Answer:
9.8 L
Explanation:
The reaction that takes place is:
- 4H₂(g) + CS₂(g) → CH₄(g)+ 2H₂S(g)
At STP, 1 mol of any gas occupies 22.4 L.
We calculate how many moles are there in 2.5 L of CH₄ at STP:
- 2.5 L ÷ 22.4 L/mol = 0.11 mol CH₄
Then we convert CH₄ moles into H₂ moles, using the stoichiometric coefficients of the reaction:
- 0.11 mol CH₄ * [tex]\frac{4molH_2}{1molCH_4}[/tex] = 0.44 mol H₂
Finally we calculate the volume that 0.44 moles of H₂ would occupy at STP:
- 0.44 mol * 22.4 L/mol = 9.8 L
