Answered

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how many liters of hydrogen gas I needed to react with CS2 to produce 2.5 L of CH4 At STP

Sagot :

maacastrobr

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
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