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3 December, 12:51

a ballon filled with helium contains 85L and 1.2 atm. the pressure is reduced to 0.22 atm at constant temperature. what is the new volume? given info: equation. work: answer

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  1. 3 December, 13:56
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    463.64L

    Explanation:

    The following data were obtained from the question:

    V1 (original volume) = 85L

    P1 (original pressure) = 1.2 atm

    P2 (new pressure) = 0.22 atm

    V2 (new volume) = ?

    Since the temperature is constant, the gas is obeying Boyle's law.

    Using the Boyle's law equation P1V1 = P2V2, the new volume of the gas can obtain as follow:

    P1V1 = P2V2

    1.2 x 85 = 0.22 x V2

    Divide both side by 0.22

    V2 = (1.2 x 85) / 0.22

    V2 = 463.64L

    Therefore, the new volume is 463.64L
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