If Δ U and Δ W represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true?

Question

If Δ U and Δ W represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true? (A) Δ U =- Δ W, in a adiabatic process (B) Δ U = Δ W, in a isothermal process (C) Δ U = Δ W, in a adiabatic process (D) Δ U = -Δ W, in a isothermal process

Tardigrade Admin · Accepted Answer

Δ U=q+W for an adiabatic process, q=0 ∴ Δ U = W i.e; increase or decrease in Internal energy is equal to work done.

Q. If $Δ U$ and $Δ W$ represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true?

$Δ U = - Δ W,$ in a adiabatic process

$Δ U = Δ W,$ in a isothermal process

$Δ U = Δ W,$ in a adiabatic process

$Δ U = - Δ W,$ in a isothermal process

$Δ U = q + W$
for an adiabatic process, $q = 0$
$∴ Δ U = W$
i.e; increase or decrease in Internal energy is equal to work done.

Q. If ΔU and ΔW represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true?

ΔU=−ΔW, in a adiabatic process

ΔU=ΔW, in a isothermal process

ΔU=ΔW, in a adiabatic process

ΔU=−ΔW, in a isothermal process