A gas with n = 0.50 mol occupies V = 11.2 L at T = 298 K. What is the pressure P (in atm) using P = nRT/V?

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Multiple Choice

A gas with n = 0.50 mol occupies V = 11.2 L at T = 298 K. What is the pressure P (in atm) using P = nRT/V?

Explanation:
The pressure is found by using the ideal gas law in the form P = nRT/V. Here, more moles and higher temperature push pressure up, while a larger volume pushes it down. Plug in the values: P = (0.50 mol) × (0.082057 L·atm/(mol·K)) × (298 K) ÷ (11.2 L). Calculating the numerator first: 0.50 × 0.082057 × 298 ≈ 12.2265 L·atm. Divide by 11.2 L to get P ≈ 1.090 atm. The units cancel to atm, as expected. So the pressure is about 1.09 atm, which corresponds to the listed option.

The pressure is found by using the ideal gas law in the form P = nRT/V. Here, more moles and higher temperature push pressure up, while a larger volume pushes it down. Plug in the values: P = (0.50 mol) × (0.082057 L·atm/(mol·K)) × (298 K) ÷ (11.2 L). Calculating the numerator first: 0.50 × 0.082057 × 298 ≈ 12.2265 L·atm. Divide by 11.2 L to get P ≈ 1.090 atm. The units cancel to atm, as expected. So the pressure is about 1.09 atm, which corresponds to the listed option.

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