Question

w - nC, (T - T) - 3 x 27,5 x 50 - 4125 Joule 10 moles of an ideal gas at 27°C and 10 atm., pressure c the following changes. Illustration 19 (1) Isothermal & reversible expansion to 246 L (ii) Isothermal and irreversible expansion to 246 L. (iii) Isochoric heating to 177°C. Calculate the work done in each transformation in Solution (i) Work done in isothermal reversible expansion V2 = -2.303 × 10 × 8. V1 w = -2.303 x nRT log = -574 (ii) Work done in isothermal irreversible expansion w = -P (V, - V,) = -1 (246 – 24.6) = -221.4 L- (iii) Work done in isochoric change Since AV =0 .. W = 0 ation 20 Find​

Answer 1

Answer:

Moles if ideal gas 10

Temprature if gas 27 degree

celcius is 300K

Pressure if ideal gas10atm

and volume of ideal gas 22.6L

1.)w=nRt lnP1/P2

=10×0.082×300× ln24624.6

=566.43J

2.)Change of volume =(246-24.6)

=2214J

3.)For isochoric process change in volume is zero

so,workdone is also zero.

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