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?
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7. Gases
The Ideal Gas Law Applications
Multiple Choice
Using the ideal gas law, what is the temperature in degrees Celsius of 5.20 moles of gas in a 40.0 L container at a pressure of 4.50 atm?
A
0 °C
B
185 °C
C
120 °C
D
273 °C
Verified step by step guidance1
Identify the known variables from the problem: number of moles \(n = 5.20\) mol, volume \(V = 40.0\) L, pressure \(P = 4.50\) atm, and the gas constant \(R = 0.0821\) L·atm/(mol·K). The temperature \(T\) in Kelvin is unknown.
Write down the ideal gas law equation: \(P \times V = n \times R \times T\).
Rearrange the ideal gas law to solve for temperature \(T\): \(T = \frac{P \times V}{n \times R}\).
Substitute the known values into the equation: \(T = \frac{4.50 \times 40.0}{5.20 \times 0.0821}\).
Calculate \(T\) in Kelvin, then convert it to degrees Celsius using the formula: \(T_{\degree C} = T_{K} - 273.15\).
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