Hello, Brandy,
I believe the question is looking for the initial temperature of a gas (O2) that is now 934.26K and went from 1.343L to 7.707L. We can use the following relationship:
P1V1/T1 = P2V2/T2,
where the subscripts 1 and 2 are the initial and final states.
Rearrnage to find T1
T1 = T2(P1/P2)(V1/V2)
The first thing that we find is that there are no values given for P1 and P2. Zounds!
We must therefore assume the pressure remains constant. P1 = P2. If so, then the (P1/P2) term cancels and so it makes no difference what the pressure is. I simply entered "1" for both pressures in the table below.
Enter the data in a table and then solve for T1, but before we start calculating, let's predict what the initial temperature might be just thinking about what happened. The volume incresed dramatically, by almost a factor of 6, or so. That means the temperature had to increase by the same factor, so I'm thinking I'll mentally round the 934,26 to 900, since I can divide that by 6 eastly enough to say I should expect a lower temperature around 150, or so.
Plug is the numbers. I get 162.8K, which gives me encouragement that this is a good answer.
I hope this helps,
Bob
Robert S.
03/15/21
BRANDY E.
Thank you! I figured it out.03/15/21