Part A: The pressure inside a hydrogen-filled container was 2.10 atm at 21 ?C. W

Question

Part A:

The pressure inside a hydrogen-filled container was 2.10 atm at 21 ?C. What would the pressure be if the container was heated to 99?C ?
Ideal gas law calculations call for temperature expressed in kelvins.

Part B:

At standard temperature and pressure (0 ?C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 90?C ?

Part C:

A balloon was filled to a volume of 2.75L when the temperature was 30.0?C. What would the volume become if the temperature dropped to 11.0?C.

Explanation / Answer

pV = nRT

A.

p1/T1 = p2/T2           (if V,n constant)

T1 = 273 + 21 = 294K

T2 = 372 K

2.1/294 = p2/372       p2 = 2.66atm

B.

V1/T1 = V2/T2   (if p,n constant)

22.4/273 = V2/363    V2 = 29.8   L

C.

V1/T1 = V2/T2

2.75/303=V2/284        V2 = 2.58L

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