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.

Question

Chemistry

Isai

2 December, 19:03

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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Answers (1)

Know the Answer?

Cruz Gentry · Answer 1

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.