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24 May, 13:39

How many grams of chlorine gas (Cl2) are in a 17.8 liter sample at 1.1 atmospheres and 29°C? Show all work used to solve this problem.

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  1. 24 May, 14:07
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    By using the ideal-gas equation: PV = nRT

    where:

    P = pressure = 1.1 atm

    V = volume = 17.8 L

    n = number of moles Cl2 (unknown)

    R = gas constant = 0.08206 L*atm/mol*K

    T = temperature = 29C + 273.15 = 302.15 K

    To calculate number of moles of Cl2

    (1.1 atm) * (17.8 L) = n * (0.08206 L*atm/mol*K) * (302.15 K)

    n = 0.79 moles Cl2

    Convert moles Cl2 to grams Cl2.

    Note: 1 mole Cl2 = 70.9064 grams Cl2

    0.79 moles Cl2 x (70.9064 grams Cl2/1 mole Cl2) = 56.0 grams Cl2
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