One more of an ideal gas at 27 degree C and 1 bar pressure is heated and allowed

Question

One more of an ideal gas at 27 degree C and 1 bar pressure is heated and allowed to expand reversibly at a constant pressure until the final temperature is 327degree C. For this gas,C _v,m = 2.5R, constant over the temperature range.(Note from SRB: C _v,m is the molar heat capacity. An earlier version of the 5th edition that I used last year used C_v with a bar over it, as we have been doing ib class, Sorry for any confussion,). Calculate the work w done on the gas in this expansion. What are delta U and delta H for the process? What is the amount of heat q adsorbed by the gas?

Explanation / Answer

A)WORK DONE by gas =R * CHANGE IN TEMPERATURE

= R * ((327+273)-(27+273))= R*300= 2490 Joules

   work done on gas is negative = -2490 J

B) delta U = Cv,m delta T= 2.5R*300= 6225 J

  delta H= delta U -delta W = 6225+2490=8715J

C)heat absorbed by gas is 8715 J

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