I did a lab today in Chemistry class and....?

Question

I have a bunch of calculations to do regarding my results. I'm stuck on a question and need help. It reads: Adjust the volume of hydrogen collected (from data table) to STP conditions. Use the COMBINED GAS LAW. P1 is the partial pressure of hyrdogen. So I need help figuring out what is what.

The partial pressure of hydrogen is 729 mmHg.

What about V1, T1, V2, P2, and T2.

I'll give the rest of my info if it helps.

0.00337 moles of Mg reacted.

0.005036 moles of hydrogen were produced

The air pressure was 748 mmHg

The air temperature was 293 degrees Kelvin

We used a 0.0109 g/cm dense Mg ribbon, (7.5 cm long)

The mass of the Mg was 0.0818 g

The volume of wet hydrogen was 0.116 L

The vapor pressure of water is 19.0 mmHg

If you need any more info to help me out, I'l be glad to add details. Thanks!

Answer 1

My last physics and chemistry classes were ages ago, so it would take me even more effort to figure this out than it would take you.  But, of course, physicists and chemists can do these sorts of things in their sleep.  Perhaps you could repost it in the physics or chemistry section?

Good luck!