Multiple Choice
A 5.00 L tank contains 2.50 moles of oxygen gas at 39.3 °C. What is the pressure in atm inside the tank? (R = 0.0821 L·atm·mol^{-1}·K^{-1})
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7. Gases
The Ideal Gas Law Applications
Multiple Choice
A balloon contains 2.0 mol of an ideal gas at a pressure of 1.0 atm and a temperature of 273 K. What volume will the balloon occupy?
A
2.0 L
B
44.8 L
C
11.2 L
D
22.4 L
Verified step by step guidance1
Identify the known variables from the problem: number of moles \(n = 2.0\) mol, pressure \(P = 1.0\) atm, and temperature \(T = 273\) K.
Recall the Ideal Gas Law equation: \(P \times V = n \times R \times T\), where \(V\) is the volume, and \(R\) is the ideal gas constant.
Choose the appropriate value for the ideal gas constant \(R\) that matches the units of pressure in atm and volume in liters, which is \(R = 0.0821 \ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K}\).
Rearrange the Ideal Gas Law to solve for volume \(V\):
\(V = \frac{n \times R \times T}{P}\)
Substitute the known values into the equation:
\(V = \frac{2.0 \ \text{mol} \times 0.0821 \ \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K} \times 273 \ \text{K}}{1.0 \ \text{atm}}\)
This will give the volume the balloon occupies.
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