A 0.982-g sample of an unknown gas exerts a pressure of 700 mm Hg in a 450-cm3 container at 23oC. Calculate the molar mass of this gas. [1cm

Question

A 0.982-g sample of an unknown gas exerts a pressure of 700 mm Hg in a 450-cm3 container at 23oC. Calculate the molar mass of this gas. [1cm3 = 1mL; 1000mL = 1L]

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Khoii Minh 6 months 2021-08-05T21:37:19+00:00 1 Answers 9 views 0

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    2021-08-05T21:38:44+00:00

    Answer:

    57.4 g/mol

    Explanation:

    Step 1: Convert 450 cm³ to L

    We will use the conversion factors 1 cm³ = 1 mL and 1000 mL = 1 L.

    450 cm³ × 1 mL/1 cm³ × 1 L/1 mL = 0.450 L

    Step 2: Convert 23 °C to Kelvin

    We will use the following expression.

    K = °C + 273.15 = 23 + 273.15 = 296 K

    Step 3: Calculate the number of moles of the gas

    We will use the ideal gas equation.

    P × V = n × R × T

    n = P × V / R × T

    n = 700 mmHg × 0.450 L / (62.4 mmHg.L/mol.K) × 296 K = 0.0171 mol

    Step 4: Calculate the molar mass of the gas

    0.982 g of the gas correspond to 0.0171 moles.

    M = 0.982 g/0.0171 mol = 57.4 g/mol

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