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17 January, 14:41

CaC2 (s) + 2H2O (l) → C2H2 (g) + Ca (OH) 2 (s).

Suppose this reaction takes place in a sealed container in which the gas occupies a volume of 1.50 liters. The container is kept at a temperature of 0°C. If 5.18 grams of calcium carbide reacts with excess water, what is the partial pressure of the ethyne gas produced, in atmospheres?

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  1. 17 January, 16:12
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    The partial pressure of the ethyne is 1.21 atmospheres.

    Explanation:

    The molar mass of calcium carbide is 64.100 grams/mole. Convert the amount of calcium carbide from grams to moles:

    5.18 g * = 0.0808 mol CaC2.

    The ratio of calcium carbide to ethyne is 1 : 1, so 0.0808 mol of ethyne is produced.

    Use the ideal gas law to find the pressure after converting the temperature to kelvins:

    0°C + 273.15 = 273 K.

    Now solve the ideal gas law formula for pressure:

    PV = nRT

    P =

    The answer needs to be in atmospheres, so use

    R = 0.0821 L atm/mol K:

    P =

    = 1.21 atm
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