A system consisting of 0.0522 moles of a diatomic ideal gas is taken from state

Question

A system consisting of 0.0522 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 0.0522 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? Where does it occur? 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) (PCVC ? PAVA) to a diatomic ideal gas. Find the energy delivered to the gas in going from A to C.

Explanation / Answer

a)as workdone during A B is 0 why because volume not changing

from BC work done is area under it

(1/2*0.3*6+0.2*6+0.3*6)

=3.9atm*l

convert it into joules

3.9*[0.001m^3][1.013*10^5pa]

=395.07j

b)pv=nrt

lowest temperature at A = (0.3*2*(0.001m^3*1.013*10^5)/8.314*0.0522)

temperature= 140k

it occurs at point A

c)change in internal energy for diatomic gas =5/2nr(t2-t1)=5/2(P1V1-P2V2)nr

from A to B = 5/2(1*8.314*0.0522)(0.001*1.013*10^5)

= 41.4j

from Bto c =99.6j

toatal = 143.6j

  

d)energy delivered = chnage in internal energy-workdone

=143.6-390.07

=-246.47j

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