A 2.00 L container holds 0.500 moles of an ideal gas at 298 K. What is the pressure?

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Multiple Choice

A 2.00 L container holds 0.500 moles of an ideal gas at 298 K. What is the pressure?

Explanation:
The pressure of an ideal gas is linked to the amount of gas, temperature, and volume by PV = nRT. Solve for P: P = nRT / V. Use R = 0.082057 L·atm/(mol·K), n = 0.500 mol, T = 298 K, V = 2.00 L. Compute nRT: 0.500 × 0.082057 × 298 ≈ 12.23 atm·L. Divide by V: 12.23 / 2.00 ≈ 6.11 atm. So the pressure is about 6.11 atm.

The pressure of an ideal gas is linked to the amount of gas, temperature, and volume by PV = nRT. Solve for P: P = nRT / V. Use R = 0.082057 L·atm/(mol·K), n = 0.500 mol, T = 298 K, V = 2.00 L.

Compute nRT: 0.500 × 0.082057 × 298 ≈ 12.23 atm·L. Divide by V: 12.23 / 2.00 ≈ 6.11 atm.

So the pressure is about 6.11 atm.

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