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9 March, 20:43

An average incandescent light bulb with a volume of 0.130 L contains 0.216 grams of argon gas. After the bulb had been burning for a few minutes, the temperature of the gas reached 100 °C.

What was the pressure of the gas at that temperature?

1.2 atm

4.01 atm

1.37 atm

0.23 atm

3.08 atm

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  1. 9 March, 22:35
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    P = 1.2 atm

    Explanation:

    Given dа ta:

    Volume = 0.130 L

    Mass of argon = 0.216 g

    Temperature = 100°C (273+100 = 373K)

    Pressure = ?

    Solution:

    Number of moles of argon:

    Number of moles = mass / molar mass

    Number of moles = 0.216 g / 40 g/mol

    Number of moles = 0.005 mol

    Pressure of argon:

    PV = nRT

    P = nRT/V

    P = 0.005 mol * 0.0821 atm. L/mol. k * 373 k / 0.130 L

    P = 0.15l * atm / 0.130 L

    P = 1.2 atm
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