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1 April, 14:45

If 345.1 g of CO2 are placed in a vessel whose volume is 32.1 L at a temperature of 20.0oC, what will the pressure be? (R = 0.0821 atm*L/mole*K)

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  1. 1 April, 14:56
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    5.88atm

    Explanation:

    First, we obtain the number of mole of CO2 present in the vessel. This is illustrated below:

    Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

    Mass of CO2 from the question = 345.1g

    Number of mole of CO2 = ?

    Number of mole = Mass/Molar Mass

    Number of mole of CO2 = 345.1/44

    = 7.84moles

    Now we can easily calculate the pressure by doing the following:

    Data obtained from the question include:

    V (volume) = 32.1 L

    T (temperature) = 20°C = 20 + 273 = 293K

    R (gas constant) = 0.0821atm*L/mole*K

    n (number of mole) = 7.84moles

    P (pressure) = ?

    We will be making use of the ideal gas equation PV = nRT to calculate the pressure

    PV = nRT

    P = nRT/V

    P = 7.84 x 0.0821 x 293/32.1

    P = 5.88atm

    Therefore, the pressure is 5.88atm
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