Combined Gas Law Equation Question Please Chemists help..?

Question

The question is at what pressure must a sample of carbon dioxide be confined in a 3.75L flask at 30degC if its volume at STP(standard conditions of temp and press) is 10.0L? The book only shows practice solutions for determining volume but not pressure. Can someone help me setup the equation so i can learn to solve for pressure?

Answer 1

Alright first you start by stating what you know about the problem. At STP you know that temp=0C, pressure=1 bar and your volume is 10 L. So this will be T1=0C, P1=1 bar, and V1=10L. Now the second situation has V2=3.75L and T2=30C. Since we know all of this, we can plug it into the combined gas law equation to determine P2. Combined Gas Law is (P1*V1)/T1=(P2*V2)/T2. If we solve for P2 we get P2=(P1*V1*T2)/(P2*T1). So plug in the values determined above and you have your answer.

Answer 2

The combined gas law equation: -
P & T must be in absolute units.
(P1xV1)/T1 = (P2xV2)/T2
P1xV1xT2 = P2xV2xT1
P1 = 1bar... P2 ?
V1 = 10.0L...V2 = 3.75L
T1 = 273K...T2 = 303K

1 x 10 x 303 = P2 x 3.75 x 273
P2 = 3030 ÷ (3.75 x 273)
P2 = 3030 ÷ 1023.75
P2 = 3bar

Answer 3

You are going to use the equation:

(P1) x (V1) / (T1) = (P2) x (V2) / (T2)

So it's going to come out to this:

(3.75 L) x (P atm) / (308 K) = (10 L) x (1 atm) / (278 K)
cross multiply :
3080 = 1042.5 P
divide to get :
P = 2.954 atm

Answer 4

The formula is PV/T =PV/T
Make sure the temperature is in kelvins.
So (10*1)/273=(P*3.75)/303
Solve for P