Multiple Choice
A sample of nitrogen dioxide gas at 130 ºC and 315 torr occupies a volume of 500 mL. What will the gas pressure be if the volume is reduced to 320 mL at 130 ºC?
11 Gases
The Ideal Gas Law Derivations
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A cylinder with a movable piston contains 0.615 moles of gas and has a volume of 295 mL. What will its volume be if 0.103 moles of gas escaped?
A
0.176 L
B
0.217 L
C
0.246 L
D
0.361 L
E
1.28 L
Verified step by step guidance1
Identify the initial conditions: The cylinder contains 0.615 moles of gas with a volume of 295 mL.
Determine the final amount of gas: Subtract the moles of gas that escaped (0.103 moles) from the initial moles (0.615 moles) to find the remaining moles of gas.
Use the ideal gas law concept: Since the pressure and temperature are constant, use the relationship \( V_1 / n_1 = V_2 / n_2 \), where \( V_1 \) and \( n_1 \) are the initial volume and moles, and \( V_2 \) and \( n_2 \) are the final volume and moles.
Rearrange the equation to solve for the final volume \( V_2 \): \( V_2 = V_1 \times (n_2 / n_1) \).
Substitute the known values into the equation: \( V_2 = 295 \text{ mL} \times ((0.615 - 0.103) / 0.615) \) and convert the final volume from mL to L by dividing by 1000.
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