4 Part Question! Five grams of nitrogen gas at an initial pressure of 3.0 atm an

Question

4 Part Question!


Five grams of nitrogen gas at an initial pressure of 3.0 atm and at 20 degrees C undergo an isobaric expansion until the volume has tripled.


A)What is the gas volume after the expansion in cm^3?

B)What is the gas temperature after the expansion? The gas pressure is then decreased at constant volume until the original temperature is reached. Answer in K

C)What is the gas pressure after the decrease? Finally, the gas is isothermally compressed until it returns to its initial volume. Answer in atm

D)What is the final gas pressure in atm?

Please show all work!

Explanation / Answer

m = 5 g, M = 28 g/mol, P1 = 3.0 atm, T1 = 20 oC = 293 K, initial volume = V1

P1V1 = mRT1/M, so V1 = mRT1/(MP1) = 1.43*103 cm3

isobaric expansion ==> P = constant, P2 = P1, V2 = 3V1
=
A)What is the gas volume after the expansion in cm^3?

V2 = 4.29*103 cm3

B)What is the gas temperature after the expansion?

V2/T2 = V1/T1

T2 = T1(V2/V1) = 3T1 = 879 K

C) The gas pressure is then decreased at constant volume until the original temperature is reached. What is the gas pressure after the decrease?

V3 = V2 = 3V1, T3 = T1, find P3

P3V3/T3 = P1V1/T1, so P3 = P1(V1/V3)(T3/T1) = P1(1/3)(1) = P1/3 = 1.0 atm

D) Finally, the gas is isothermally compressed until it returns to its initial volume. What is the final gas pressure in atm?

note V4 = V1, T4 = T

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