First Law of Thermodynamics
The amount heat absorbed by the system is equal to the change in it’s interval energy and work done by the system.
It is the consequence of conservation of energy for gaseous system.
Heat supplied to the gas = Increase in internal energy + work done by the gas.
Q=ΔU+W Q=+ve ⇒ heat is supplied to the gas
in differential form dQ=dU+dW Q=-ve⇒heat is taken out from the gas
and dQ=nCdT = molar specific heat
C=C_P (constant pressure); C=C_v =(constant volume)
and dU=d[(f/2)nRT] f = degree of freedom
dU=(f/2)nRdT dU=+ve for increase in temperature
dU=–ve for decrease in temperature
dW=∫_(V_1)^(V_2)▒PdV (P = pressure of the gas of which work is to be calculated)
W=+ve for work done by gas (in expansion of gas)
W=–ve for work done by gas (in contraction of gas)
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