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8 August, 06:39

A 500 mL sample of a gas at 507 torr and 97 Degrees Celcius has a mass of 0.966g. What is the gas?

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  1. 8 August, 06:48
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    the gas is identified as follows

    by use of ideal gas equation that is PV = nRT where n is number of moles calculate the number of moles involved

    P = 507 torr

    R (gass constant) = 62.364 L. torr/K. mol

    T = 97 + 273 = 370 k

    V = 500ml = 500/1000 = 0.5 Liters

    by making n the subject of the formula n = PV/RT

    = (507 torr x0.5 L) / 62.364 L. torr/Mol. k x 370 k) = 0.011 moles

    the molar mass of the gas = mass / number of moles

    = 0.966/0.011 = 88 g/mol = the gas is therefore Krypton since 88 g/mol is one of the isotope of krypton
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