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17 June, 03:05

If 22.9 g of solid carbon dioxide was placed in a similar container already containing air at 720. torr, what would be the partial pressure of carbon dioxide and the total pressure in the container after the carbon dioxide had vaporized?

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  1. 17 June, 04:49
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    ppCO2 = 1.51 atm

    total pressure = 3atm

    Explanation:

    The reaction involved is C + O2 = CO2

    I need the number of moles to be able to calculate the partial pressure of CO2 with the general equation of gases.

    n = 22.9gCO2 * (1molCO2 / 44gCO2) = 0.52mol

    T = 20 ° + 273.15K = 293.15K

    V = 22.4L

    p = nRT / V = (0.52mol * (0.082 atm * L / K * mol) * 293.15K) / 22.4L

    ppCO2 = 0.56 atm

    ppaire = 720torr * (1 atm / 760torr) = 0.95atm

    total pressure = ppCO2 + ppaire = 0.56 + 0.95

    total pressure = 1.51atm
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