[Efrem22]

I'm once again not 100% if I'm doing this right and just want some opinions/guidance if it isn't right.

1. I have 2.98atm and need to convert it to kPa.

I did - 2.98*101,325/1atm = 301,948.6 kPa

2. a sample of helium gas occupies 33L @ 47 degC and .956 atm. What volume (L) will it occupy at 85 degC and .956atm?

I did 47degC -> 320K
       85degC -> 358K

V1/T1 = V2/T2

33l*358/320 = 36.9L

3. 33mol of CO2 is stored in a balloon at STP - what is the volume of the balloon?

I used V=MRT/P

V= 33mol*0.0821L*1atm/k*273K/1atm
V= 739.6L

Do any of these seem right at all?
Thanks

[Efrem22]

Nevermind about those questions, I found out that they were good. But I do have another question that I have no idea how to answer.


The largest a party balloon can get before bursting is 75L at 37C and 1.00atm. Suppose you fill the balloon with O2 gas. How many grams of oxygen can be added to the balloon before it pops? Assuming the balloon had no gas in it before the oxygen is added.

[vhpk]

Nevermind about those questions, I found out that they were good. But I do have another question that I have no idea how to answer.


The largest a party balloon can get before bursting is 75L at 37C and 1.00atm. Suppose you fill the balloon with O2 gas. How many grams of oxygen can be added to the balloon before it pops? Assuming the balloon had no gas in it before the oxygen is added.

What's the condition for using ideal gas law?
What do you need to calculate the mass of oxygen?