Based on the first law of thermodynamics, which one of the following is correct?

Question

Based on the first law of thermodynamics, which one of the following is correct? (A) For an isochoric process= Δ E=-Q (B) For an adiabatic process= Δ E=-W (C) For an isothermal process= Q=+W (D) For a cyclic process= Q=-W

Tardigrade Admin · Accepted Answer

The mathematical equation for first law of thermodynamics is,

Δ E = Q + W

(a) For isochoric process,

Δ V = 0

W = - P_{e x t} Δ V = 0

∴

Δ E = Q

(b) For adiabatic process,

Q = 0

Δ E = W

(c) For isothermal process,

Δ T = 0

and

Δ E = 0

Q = - W

(d) For cyclic process, state functions like

Δ E = 0

Q = - W

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

For an isochoric process= $Δ E = - Q$

For an adiabatic process= $Δ E = - W$

For an isothermal process= $Q = + W$

For a cyclic process= $Q = - W$

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

For an isochoric process= ΔE=−Q

For an adiabatic process= ΔE=−W

For an isothermal process= Q=+W

For a cyclic process= Q=−W

The mathematical equation for first law of thermodynamics is, ΔE=Q+W (a) For isochoric process, ΔV=0 W=−Pext​ΔV=0 ∴ ΔE=Q (b) For adiabatic process, Q=0 ΔE=W (c) For isothermal process, ΔT=0 and ΔE=0 Q=−W (d) For cyclic process, state functions like ΔE=0 Q=−W

For an isochoric process= $Δ E = - Q$

For an adiabatic process= $Δ E = - W$

For an isothermal process= $Q = + W$

For a cyclic process= $Q = - W$