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jasonr182017
31.01.2020 •
Chemistry
Part 1. determine the molar mass of a 0.458-gram sample of gas having a volume of 1.20 l at 287 k and 0.980 atm. show your work. part 2. if this sample was placed under extreme pressure, describe how the actual volume would compare to the predicted volume. explain your answer.
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Ответ:
Part 1: 9.165 g/mol.
Part 2: The volume will decrease.
Explanation:
Part 1:
To solve this problem, we can use the general gas law:PV = nRT,
where, P is the pressure of the gas (atm) (P = 0.98 atm).
V is the volume of the gas (L) (V = 1.2 L).
n is the no. of moles of the gas (mol).
R is the general gas constant (R = 0.082 L.atm/mol.K).
T is the temperature of the gas (K) (T = 287 K).
∴ n = PV/RT = (0.98 atm)(1.2 L)/(0.082 L.atm/mol.K)(287 K) = 0.0499 mol ≅ 0.05 mol.
∵ n = mass/molar mass
∴ molar mass = mass/n = (0.458 g)/(0.05 mol) = 9.165 g/mol.
Part 2:
The volume of the gas will decrease as the sample is placed under extreme pressure.
Boyle’s Law states that at constant temperature, the volume of a given quantity of a gas varies inversely with its pressure.
P ∝ 1/V.
so, as the sample is placed under extreme pressure, the volume of the gas will be decreased.
Ответ:
I don't know what you're talking about. But I hope they forgive you. <3
Explanation: