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    I'm going through a past paper I sat last summer & I can't find the mark scheme so I was wondering if anyone could help me with this question because I don't know if my answer is correct

    On adding a strip of Mg to HCl acid, 125cm^3 of hydrogen gas formed at temp 24 degrees Celsius and a pressure of 1.01x10^5 Pa. Calculate the volume occupied by this has under the same pressure and at a temp of 52 degrees Celsius.
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    pV = nRT

    You can rearrange the ideal gas law into:
    p/(nR) = T/V
    Since the amount of hydrogen (n), the pressure (p) and, obviously, R remain constant, p/(nR) is the same at both temperatures.

    Therefore:
    T1/V1 = T2/V2 (which you might have called Charles' law)

    Final volume = 270 cm3 (2 d.p.)
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    (Original post by zoae)
    pV = nRT

    You can rearrange the ideal gas law into:
    p/(nR) = T/V
    Since the amount of hydrogen (n), the pressure (p) and, obviously, R remain constant, p/(nR) is the same at both temperatures.

    Therefore:
    T1/V1 = T2/V2 (which you might have called Charles' law)

    Final volume = 270 cm3 (2 d.p.)
    Thank you!!
 
 
 
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