Five grams of nitrogen gas at an initial pressure of 3.0 atm and at 20 degree C

Question

Five grams of nitrogen gas at an initial pressure of 3.0 atm and at 20 degree C undergo an isobaric expansion until the volume has tripled. What is the gas volume alter the expansion? Express your answer with the appropriate units. What is the gas temperature after the expansion (in degree C)? Express your answer with the appropriate units. The gas pressure is then decreased at constant volume until the original temperature is reached. What is the gas pressure after the decrease? Express your answer with the appropriate units. Finally, the gas is isothermally compressed until it returns to its initial volume. What is the final gas pressure? Express your answer with the appropriate units.

Explanation / Answer

using the universal gas law we have

PV = nRT

3*V = (5/28) * (0.0821)*(273+20)

V = 1.43 L

the volume has tripled after expansion V(new) =3V = 3*1.43 = 4.29 L = 4290 cm3

b) V1/T1 = V2/T2

V/293 = 3V/T2

T2 = 3*293 = 879 K = (879-273) = 606oC

C) P1/T1 = P2/T2

3 / 879 = P2 / 293

P2 = 1 atm

D) P1V1 = P2V2

1*4290 = P2* 1430

P2 = 3 atm

final gas pressure = 3 atm

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