Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas ? (Assume non-expansion work is zero)

Question

Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas ? (Assume non-expansion work is zero) (A) Cyclic process: q = - w (B) Isothermal process: q = - w (C) Adiabatic process: Δ U = - w (D) Isochoric process: Δ U = q

Tardigrade Admin · Accepted Answer

For cyclic process: Δ U = 0 ⇒ q = - w For isothermal process: Δ U = 0 ⇒ q = - w For adiabatic process: q = 0 ⇒ Δ U = W For isochoric process: w = 0 ⇒ Δ U = q

Q. Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas ? (Assume non-expansion work is zero)

Cyclic process : $q = - w$

Isothermal process : $q = - w$

Adiabatic process : $Δ U = - w$

Isochoric process : $Δ U = q$

For cyclic process : $Δ U = 0 \Rightarrow q = - w$
For isothermal process : $Δ U = 0 \Rightarrow q = - w$
For adiabatic process : $q = 0 \Rightarrow Δ U = W$
For isochoric process : $w = 0 \Rightarrow Δ U = q$

Q. Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas ? (Assume non-expansion work is zero)

Cyclic process : q=−w

Isothermal process : q=−w

Adiabatic process : ΔU=−w

Isochoric process : ΔU=q

For cyclic process : ΔU=0⇒q=−w For isothermal process : ΔU=0⇒q=−w For adiabatic process : q=0⇒ΔU=W For isochoric process : w=0⇒ΔU=q

Cyclic process : $q = - w$

Isothermal process : $q = - w$

Adiabatic process : $Δ U = - w$

Isochoric process : $Δ U = q$

For cyclic process : $Δ U = 0 \Rightarrow q = - w$
For isothermal process : $Δ U = 0 \Rightarrow q = - w$
For adiabatic process : $q = 0 \Rightarrow Δ U = W$
For isochoric process : $w = 0 \Rightarrow Δ U = q$