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Based on first Jaw of thermodynamics which of the following is correct
  • a)
    for an isobaric process, qp = ΔU + w
  • b)
    for an adiabatic process, ΔU = -w
  • c)
    for an isochoric process, ΔU = -qv
  • d)
    for an isothermal process, q = + w
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
Based on first Jaw of thermodynamics which of the following is correc...
In the isobaric process, pressure is constant, and volume increases from V1 to V2 due to heat absorption. According to the first law of thermodynamics, ΔU = q + W
At constant pressure, qp = ΔU -W.
qp = ΔU - pΔV
qp = U2 - U1 - (-p(V2 - V1))
qp = (U2 + pV2) - (U1 + pV1)
qp = H2 - H1
qp = ΔH
As we know, ΔH = ΔU + pΔV
ΔH = ΔU + W
Putting the value of ΔH in (1)
qp = ΔU + W
Other corrected options are as follows:
  • For adiabatic process ΔU = W
  • For an isochoric process ΔU = qv
  • For an isothermal process q = -W
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Based on first Jaw of thermodynamics which of the following is correcta)for an isobaric process, qp = ΔU + wb)for an adiabatic process, ΔU = -wc)for an isochoric process, ΔU = -qvd)for an isothermal process, q = + wCorrect answer is option 'A'. Can you explain this answer?
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