A 3.9-L volume of ideal neon gas (monatomic)is at a pressure of 5.6 aym and a temperature of 330 K. The atomic mass of neon is 20.2 g/mol. The temperature of the gas is now increased to 430 K and the volume is increased to 5.9 L.
What is the final pressure of the gas?

Question

A 3.9-L volume of ideal neon gas (monatomic)is at a pressure of 5.6 aym and a temperature of 330 K.  The atomic mass of neon is 20.2 g/mol. The temperature of the gas is now increased to 430 K and the volume is increased to 5.9 L. 
What is the final pressure of the gas?

Quizplus · Accepted Answer

Using the ideal gas law and the combined gas law, $P_1V_1/T_1 = P_2V_2/T_2$, where $P_1 = 5.6 \, \text{atm}$, $V_1 = 3.9 \, \text{L}$, $T_1 = 330 \, \text{K}$, $V_2 = 5.9 \, \text{L}$, and $T_2 = 430 \, \text{K}$. Solving for $P_2$, $P_2 = (P_1V_1/T_1) \times (T_2/V_2) = (5.6 \times 3.9 / 330) \times (430 / 5.9) = 4.8 \, \text{atm}$.

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