A 2.00 L container holds 0.800 moles of an ideal gas at 298 K. What is the pressure?

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Multiple Choice

A 2.00 L container holds 0.800 moles of an ideal gas at 298 K. What is the pressure?

Explanation:
This question tests how to use the ideal gas law to relate pressure, volume, amount, and temperature. The pressure is found from P = nRT / V. Using n = 0.800 mol, R = 0.082057 L atm / (mol K), T = 298 K, and V = 2.00 L: P = (0.800 mol)(0.082057 L atm / (mol K))(298 K) / (2.00 L) ≈ 9.78 atm. So the pressure is about 9.8 atm. The other numbers are far from this value given the same n, V, and T, so they don’t match the calculated result.

This question tests how to use the ideal gas law to relate pressure, volume, amount, and temperature. The pressure is found from P = nRT / V.

Using n = 0.800 mol, R = 0.082057 L atm / (mol K), T = 298 K, and V = 2.00 L:

P = (0.800 mol)(0.082057 L atm / (mol K))(298 K) / (2.00 L) ≈ 9.78 atm.

So the pressure is about 9.8 atm. The other numbers are far from this value given the same n, V, and T, so they don’t match the calculated result.

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