Multiple Choice
A sample of gas occupies 25.0 L at 100°C and constant pressure. What volume will the gas occupy at 200°C, assuming ideal gas behavior?
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7. Gases
The Ideal Gas Law Applications
Multiple Choice
A student collects a gas over water in a closed container. The atmospheric pressure is patmos = 1.00 atm, and the vapor pressure of water at the experimental temperature is 0.030 atm. What is the pressure of the dry gas (pgas) in the container?
A
1.00 atm
B
1.03 atm
C
0.030 atm
D
0.97 atm
Verified step by step guidance1
Understand that the total pressure inside the container is the sum of the pressure of the dry gas and the vapor pressure of water because the gas is collected over water. This is expressed as: \(P_{\text{total}} = P_{\text{gas}} + P_{\text{water vapor}}\).
Identify the given values: atmospheric pressure \(P_{\text{atmos}} = 1.00\) atm, which equals the total pressure \(P_{\text{total}}\), and the vapor pressure of water \(P_{\text{water vapor}} = 0.030\) atm.
Rearrange the equation to solve for the pressure of the dry gas: \(P_{\text{gas}} = P_{\text{total}} - P_{\text{water vapor}}\).
Substitute the known values into the equation: \(P_{\text{gas}} = 1.00\ \text{atm} - 0.030\ \text{atm}\).
Calculate the difference to find the pressure of the dry gas, which represents the pressure exerted by the collected gas excluding water vapor.
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