I have a packet of homework so I think I may post other questions that I'm stuck on later this weekend. So that's a heads up.

This packet deals with Gas Laws.

1. Given 100 ml of dry gas measured at 37° C and 760 mmHg, what would be its volume at 60°C?

I used Charle's Law and solved for V2.

So... (100/310)(333)=107.4ml

correct?

2. Given 100 ml of dry gas at 37°C and 760 mmHg, what would be its volume at 60°C and 800 mmHg?

I used the combined gas law and solved for V2.

So... (760)(100)(333)/(310)(800)=102ml

3. Given 325 ml of saturated gas at 760 mmHg and 25°C, what would be its volume if dry at the same pressure and temperature?

I got confused when I read 'if dry' Does that mean I have to subtract something out of 760mmHg?
And would I used the combined gas law and solved for V2?

Thanks!

1. yes

2. yes
3. There will be less gas when the saturated gas is dried. Subtract the vapor pressure of water at 25 C (23.8 mm Hg) from the 760 mmHg pressure to get the initial dry gas partial pressure. Since the pressure is maintained at 760 mm, that means the volume must be reduced by the fraction (760- initial water vapor pressure)/760

Can you explain to me how you got the vapor pressure of water, the 23.8mmHG?

How did you get that number?

And so the final number component is 0.96?

You have to look up the vapor pressure. See

http://genchem1.chem.okstate.edu/1314SP06/Database/VPWater.html
for example.
Assuming that the gas was saturqated with H2O, the final volume is reduced to 96.9% of the initial volume, or 315 ml.

30 cubic meters of argon gas are kept under constant pressure. The gas is heated from 10.0 degrees Celsius to 293 degrees Celsius. What is the new volume of the gas?

For question 1, you correctly used Charles's Law to solve for the volume at 60°C. Charles's Law states that at constant pressure, the volume of a gas is directly proportional to its temperature. So, by using the equation V1/T1 = V2/T2, where V1 is the initial volume (100 ml), T1 is the initial temperature (37°C), T2 is the final temperature (60°C), and V2 is the final volume which you're solving for, you got the correct answer of 107.4 ml. Well done!

For question 2, you used the combined gas law correctly. This law allows you to calculate the final volume (V2) when given the initial volume (V1), initial temperature (T1), final temperature (T2), initial pressure (P1), and final pressure (P2). The equation is P1V1/T1 = P2V2/T2. By plugging in the given values, you obtained 102 ml as the final volume. Great job!

Regarding question 3, when it says "if dry," it means that you need to find the volume of the gas assuming it is completely dry and not saturated with water vapor. Since the pressure and temperature are provided, you can use the ideal gas law equation PV = nRT to solve for the volume (V), where P is the pressure (760 mmHg), V is the volume (which you're solving for), n is the number of moles (which remains constant), R is the ideal gas constant, and T is the temperature (25°C converted to Kelvin). You do not need to subtract anything from the given pressure. Please note that the ideal gas law assumes non-condensed gases.