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23 May, 09:41

A gas sample has an original volume of 760 ml when collected at 700 mm and 40oC. If a change is made in the gas temperature which causes the volume of the gas sample to become 420 ml at 1.25 atm, what is the new temperature?

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  1. 23 May, 12:17
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    235k

    Explanation:

    To solve this problem, we will use the general gas equation.

    In its simplest form, the general gas equation can be represented as follows:

    P1V1/T1 = P2V2/T2

    P1 = 700mmHg

    V1 = 760ml

    T1 = 40 degrees Celsius = 40 + 273.15 = 313.15K (conversion into standard temperature unit)

    P2 = 1.25 atm

    We have to covert this into the same unit as the first pressure.

    760mmHg = 1atm

    x mmHg = 1.25 atm

    x = 1.25 * 760 = 950mmHg

    V2 = 420ml

    T2 = ?

    Now, rearranging the equation will yield:

    T2 = P2V2T1/P1V1

    T2 = 950 * 420 * 313.5/700 * 760

    T2 = 235.125K or - 38.025 degrees celcius
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