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

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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

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RobertKer 3 months 2021-07-29T14:29:47+00:00 1 Answers 14 views 0

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    2021-07-29T14:31:04+00:00

    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 * \frac{4molH_2}{1molCH_4} = 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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