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17 May, 10:31

A gas mixture is made up of kr (21.7 g), o2 (7.18 g), and co2 (14.8 g). the mixture has a volume of 23.1 l at 59 °c. calculate the partial pressure of each gas in the mixture and the total pressure of the gas mixture.

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  1. 17 May, 11:03
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    Answer: - partial pressure of Kr = 0.306 atm, partial pressure of oxygen = 0.264 atm and partial pressure of carbon dioxide = 0.396 atm

    Total pressure is 0.966 atm

    Solution: - moles of Kr = 21.7 g x (1mol/83.8g) = 0.259 mol

    moles of oxygen = 7.18 g x (1mol/32g) = 0.224 mol

    moles of carbon dioxide = 14.8 g x (1mol/44g) = 0.336 mol

    Volume of container = 23.1 L and the temperature is 59 + 273 = 332 K

    From ideal gas law equation, P = nRT/V

    partial pressure of Kr = (0.259 x 0.0821 x 332).23.1 = 0.306 atm

    partial pressure of oxygen = (0.224 x 0.0821 x 332) / 23.1 = 0.264 atm

    partial pressure of carbon dioxide = (0.336 x 0.0821 x 332) / 23.1 = 0.396 atm

    Total pressure of the gas mixture = 0.306 atm + 0.264 atm + 0.396 atm = 0.966 atm
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