From the definitions , it is clear that two heat capacities
are not equal and CP is greater than CV by a factor which
is related to the work done. At a constant pressure part of heat absorbed by
the system is used up in increasing the internal energy of the system and the
other for doing work by the system. While at constant volume the whole of heat
absorbed is utilized in increasing the temperature of the system as there is no
work done by the system. Thus increase in temperature of the system would be
lesser at constant pressure than at constant volume. Thus CP is
greater than Cv.
We know Cp
= dH/dT …(1)
And Cv
= dE/dT ….(2)
By definition, H = E + PV for 1 mole of an ideal gas
Or H = E + RT (PV= RT)
Differentiating w.r.t. temperature, T, we get
dH/dT
= dE/dT + R
or Cp
= Cv+ R By
using (1) and (2)
or Cp
– Cv = R
(Shown)
please show that using maxwell relation
ReplyDeleteThis is an incomplete proof. dH/dT and dE/dT are partial derivatives. So you could have (dH/dT)p (dE/dT)p --or-- (dH/dT)v (dU/dT)v
ReplyDeletefor the approach in our solution, you need to show that (dE/dT)p=(dE/dT)v
your*
ReplyDeleteexplanation is clear but some not catch that ,so give every reactions breifly . not only thse all organic reactions
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ReplyDeleteja a6e ta tei hoye jabe...
ReplyDeleteVlo na ata
DeleteVlo na ata
DeleteVery good explanation.
ReplyDeleteSir can you please give a graph for the reaction
ReplyDeleteSuperb explanation sir
ReplyDeleteThanku so much for your efforts.