Multiple Choice
In experiment 1, a sample of propane gas occupies 75.0 mL at constant temperature. If the initial pressure was 1.20 atm at 100.0 mL, what would be the pressure of the propane gas at 75.0 mL?
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7. Gases
The Ideal Gas Law Applications
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})
A
10.1 atm
B
8.2 atm
C
14.0 atm
D
13.2 atm
Verified step by step guidance1
Identify the known variables from the problem: number of moles \(n = 2.50\) mol, volume \(V = 5.00\) L, temperature \(T = 39.3\ ^\circ\mathrm{C}\), and the gas constant \(R = 0.0821\ \mathrm{L \cdot atm \cdot mol^{-1} \cdot K^{-1}}\).
Convert the temperature from Celsius to Kelvin using the formula: \(T(K) = T(^\circ C) + 273.15\). So, calculate \(T = 39.3 + 273.15\) K.
Use the Ideal Gas Law equation to relate pressure, volume, moles, and temperature: \(P V = n R T\).
Rearrange the Ideal Gas Law to solve for pressure \(P\): \(P = \frac{n R T}{V}\).
Substitute the known values of \(n\), \(R\), \(T\) (in Kelvin), and \(V\) into the equation and calculate the pressure \(P\) in atm.
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