Chemistry ASAP!!!

Question

1.) A 5.15L balloon has a pressure of 1.35 atm if compressed to 3.43L what will be the resulting pressure?

2.) 0.785 moles of N2 fill a balloon at 1.5atm and 301K. What is the volume of the balloon?

Answer 1

Using Ideal Gas law:

P1 = 1.45 atm

V1 = 5.15 L

P2 = ?

V2 = 3.43 L

Using Ideal Gas Law, PV = nRT:

Now, the number of moles (n) are the same regardless of pressure and volume, let's assume that the temperature is constant since there is no information given in the problem. Therefore,

P1V1 = nRT = P2V2

P1V1 = P2V2

Solve for P2 and you get 2.03 atm. This makes sense because you reduce the volume of a gas by compressing it, which means you are increasing the pressure.

2) P = 1.5 atm

T = 301 K

n = 0.785 moles

PV = nRT

V = nRT/P

R = 0.0821 (L*atm)/(mol * K)

Therefore,

V = (0.785 * 0.0821 * 301)/1.5 = 19.4 L