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A sample of 2.00 moles of gas initially at STP is converted to volume of 5.0 L & temperature of 27 degrees C?

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What is its new pressure in atm?

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  1. STP = 1atmosphere pressure and 273 Kelvin temperature (0°C).

    1 mole at STP = 22.4 Litres Volume.

    2 moles therefore = 44.8 Litres.

    Using the Combined Gas Law..

    P1:1.0atm x V1:44.8L x T2:300K. = P2:? x V2:5.0L x T1:273K

    New Pressure (P2) = (1 x 44.8 x 300) / (5 x 273)

    = 13,440 / 1,365

    = a)...9.8 atmospheres pressure.


  2. PV=nRT

    1xV=2x0.08206x273

    V = 44.804 L

    PV/T = P1V1/T1

    1x44.804/273 = Px5.0/300

    P = 2816 atm

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