Based on first law of thermodynamics which of the following is correct

Question

Based on first law of thermodynamics which of the following is correct (A) for an isobaric process, qp = Δ U + w (B) for an adiabatic process, Δ U = -w (C) for an isochoric process, Δ U = -qv (D) For an cyclic process, W =- Q

Tardigrade Admin · Accepted Answer

When a system returns to its original state after completing a series of changes, then it is known that a cycle is completed. This process is known as cyclic process. In a cyclic process the initial and the final state is same. As the internal energy U of the system depends only on the state of the system so in a cyclic process the net change of internal energy, Δ U will be equal to zero i.e. Δ U =0. Hence from the first law (Δ U=Q+W) Hence, W=-Q

Q. Based on first law of thermodynamics which of the following is correct

for an isobaric process, $q_{p} = Δ U + w$

for an adiabatic process, $Δ U = - w$

for an isochoric process, $Δ U = - q_{v}$

For an cyclic process, $W = - Q$

Q. Based on first law of thermodynamics which of the following is correct

for an isobaric process, qp​=ΔU+w

for an adiabatic process, ΔU=−w

for an isochoric process, ΔU=−qv​

For an cyclic process, W=−Q

for an isobaric process, $q_{p} = Δ U + w$

for an adiabatic process, $Δ U = - w$

for an isochoric process, $Δ U = - q_{v}$

For an cyclic process, $W = - Q$