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3 September, 14:20

A 3.25 liter container of ammonia gas exerts a pressure of 652 mm Hg at a temperature of 243 Kelvin. Calculate the pressure of this same amount of gas in a 2.50 Liter container at a temperature of 221 Kelvin

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  1. 3 September, 16:26
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    1.01atm

    Explanation:

    First, we need to calculate the numbers of mol of ammonia. This can be achieved by doing the following:

    V = 3.25L

    P = 652mmHg we must convert this to atm by:

    760mmHg = 1atm

    652mmHg = 652/760 = 0.858atm

    T = 243K

    R = 0.082atm. L/K / mol

    n = ?

    PV = nRT

    n = PV / RT

    n = (0.858 x 3.25) / (0.082x243)

    n = 0.14mol

    From the question, we were to that the other gas had the same amount (0.14mol) as ammonia. We can calculate for the pressure of the gas as illustrated below:

    P = ?

    V = 2.5L

    T = 221K

    R = 0.082atm. L/k/mol

    n = 0.14mol

    PV = nRT

    P = nRT / V

    P = (0.14x0.082x221) / 2.5

    P = 1.01atm
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