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

Question

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

Tardigrade Admin · Accepted Answer

Δ U = q + w for an isothermal process, Δ U =0, q =- W for an isochoric process; W=0, Δ U=q for an adiabatic process, q =0, Δ U = W for a cyclic process, Δ U =0 q=-w

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

For an isothermal process, q =+ w

For an isochoric process, $Δ U = - q$

For an adiabatic process, $Δ U = - w$

For a cyclic process, q=-w

$Δ U = q + w$

for an isothermal process, $Δ U = 0, q = - W$

for an isochoric process; $W = 0, Δ U = q$

for an adiabatic process, $q = 0, Δ U = W$

for a cyclic process, $Δ U = 0$

$q = - w$

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

For an isothermal process, q =+ w

For an isochoric process, ΔU=−q

For an adiabatic process, ΔU=−w

For a cyclic process, q=-w

ΔU=q+w for an isothermal process, ΔU=0,q=−W for an isochoric process; W=0,ΔU=q for an adiabatic process, q=0,ΔU=W for a cyclic process, ΔU=0 q=−w

For an isochoric process, $Δ U = - q$

For an adiabatic process, $Δ U = - w$

$Δ U = q + w$

for an isothermal process, $Δ U = 0, q = - W$

for an isochoric process; $W = 0, Δ U = q$

for an adiabatic process, $q = 0, Δ U = W$

for a cyclic process, $Δ U = 0$

$q = - w$