Question

What is the volume of 1.0 mol of an ideal gas at standard temperature and pressure (STP)? (STP is 0°C and 1.0 atm, and the ideal gas constant R = 0.0821 L·atm/mol·K)

• A. \( 22.4 \, \text{L} \)
• B. \( 24.0 \, \text{L} \)
• C. \( 20.0 \, \text{L} \)
• D. \( 25.0 \, \text{L} \)

Hint:

At standard temperature and pressure (STP), \( 1 \, \text{mol} \) of an ideal gas occupies a volume of \( 22.4 \, \text{L} \). This is a key value to remember for ideal gas calculations at STP.

Answer 1

The Correct Option is A

At STP, the volume of \( 1 \, \text{mol} \) of an ideal gas is given by the ideal gas law: \[ PV = nRT \] Where: - \( P = 1.0 \, \text{atm} \) (pressure), - \( V \) is the volume, - \( n = 1.0 \, \text{mol} \) (amount of gas), - \( R = 0.0821 \, \text{L·atm/mol·K} \) (gas constant), - \( T = 273.15 \, \text{K} \) (temperature in Kelvin, since \( 0^\circ C = 273.15 \, \text{K} \)). Rearranging the ideal gas law to solve for \( V \): \[ V = \frac{nRT}{P} \] Substitute the values: \[ V = \frac{1.0 \times 0.0821 \times 273.15}{1.0} \] \[ V = 22.4 \, \text{L} \] Thus, the volume of \( 1.0 \, \text{mol} \) of an ideal gas at STP is \( 22.4 \, \text{L} \).