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30 June, 09:04

What is the density of a sample of ammonia gas (NH 3) if the pressure is 705 mm Hg and the temperature is 63.0°C?

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  1. 30 June, 10:38
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    Density of the gas = 0.57 g/L

    Explanation:

    We can solve this, by the Ideal Gases Law.

    We know by Avogadro's Law that 1 mol of any gas will occupy the same volume if we measure the same temperature and pressure conditions.

    1 mol of Ideal Gas occupies 22.4 L at STP (1 atm and 273K)

    We can compare the two situations to determine the volume for the second one.

    We convert the T° and the pressure

    705 mmHg. 1 atm / 760 mmHg = 0.927 atm

    63°C + 273 = 336 K

    As n and R are the same, we have: P₁. V₁ / T₁ = P₂. V₂ / T₂

    1 atm. 22.4L / 273K = 0927 atm. V₂ / 336K

    (1 atm. 22.4L / 273K). 336 K = 0.927 atm. V₂

    27.5 atm. L / 0.927 atm = V₂ → 29.7 L

    1 mol of ammonia weighs 17 g

    Density of the gas → mass / volume → 17 g / 29.7L = 0.57 g/L
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