A system consisting of 0.0192 moles of a diatomic ideal gas is taken from state

Question

A system consisting of 0.0192 moles of a diatomic ideal gas is taken from state A to state C along the path in the figure below.

3 2 A system consisting of 0.0192 moles of a diatomic ideal gas is taken from state A to state C along the path in the figure below. How much work is done on the gas during this process? What is the lowest temperature of the gas during this process? Find the change in internal energy of the gas in going from A to C. Hint: Adapt the equation (for the change in internal energy of a monatomic ideal gas) Find the energy delivered to the gas in going from A to C.

Explanation / Answer

n = 0.0192

a) workdone, W = area under the curve

W = 0.5*(0.8-0.5)*1.013*10^5*(8-2)*10^-3 + 0.5*1.013*10^5*(8-2)*10^-3


= 395.07 J

b) at point A the system will have lowest temperature

P*V = n*R*T

T = P*V/(n*R)

= 0.3*1.013*10^5*2*10^-3/(0.0192*8.314)

= 380.75 K

c)
for diatomic gas

delta U = (5/2)*(Pc*Vc - PA*VA)

= 2.5*(0.5*1.013*10^5*8*10^-3 - 0.3*1.013*10^5*2*10^-3)

= 861.05 J

d)

Q = W + delta U

= 395.07 + 861.05

= 1256.12

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