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22 May, 12:28

On a day when the barometer reads 75.23 cm, a reaction vessel holds 250 mL of ideal gas at 20 celsius. An oil manometer (rho = 810 kg/m^3) reads the pressure in the vessel to be 41 cm of oil and below atmospheric pressure. What volume will the gas occupy under S. T. P.?

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  1. 22 May, 12:49
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    V2 = 8.25 ml

    Explanation:

    First we will list down the data that is given to us:

    V1 = 250 ml

    T1 = 20° C + 273K = 293K

    T2 = 25° C + 273K = 298K (AT STP)

    Density at STP = 13600 kg/m^3

    First we will calculate the pressure inside the vessel using the formula

    P = (ρ) (g) (h)

    P1 = (810) (9.8) (0.41)

    P1 = 3254.58 pa

    P2 = (13600) (9.8) (0.7523)

    P2 = 100266.544 pa

    Now in order calculate the volume that the gas occupies we will use the following formula,

    (P1*V1) / T1 = (P2*V2) / T2

    Making V2 as the subject of the equation we get,

    V2 = (P1*V1*T2) / (P2*T1)

    V2 = (3254.58*250*298) / (100266.544*293)

    V2 = 8.25 ml
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