During isothermal expansion of an ideal gas, its

Question

During isothermal expansion of an ideal gas, its (A) internal energy increases (B) enthalpy decreases (C) enthalpy remains unaffected (D) enthalpy reduces to zero

Tardigrade Admin · Accepted Answer

During isothermal expansion of an ideal gas, Δ T=0. Now H=E+P V ∵ Δ H=Δ E+Δ(P V) ∴ Δ H=Δ E+Δ(n R T) Thus if Δ T=0 ., Δ H=Δ E i.e., remain unaffected

Q. During isothermal expansion of an ideal gas, its

internal energy increases

enthalpy decreases

enthalpy remains unaffected

enthalpy reduces to zero

During isothermal expansion of an ideal gas, $Δ T = 0$ .
Now $H = E + P V$
$∵ Δ H = Δ E + Δ (P V)$
$∴ Δ H = Δ E + Δ (n RT)$
Thus if $Δ T = 0., Δ H = Δ E$
i.e., remain unaffected

Q. During isothermal expansion of an ideal gas, its

internal energy increases

enthalpy decreases

enthalpy remains unaffected

enthalpy reduces to zero

During isothermal expansion of an ideal gas, ΔT=0. Now H=E+PV ∵ΔH=ΔE+Δ(PV) ∴ΔH=ΔE+Δ(nRT) Thus if ΔT=0.,ΔH=ΔE i.e., remain unaffected

During isothermal expansion of an ideal gas, $Δ T = 0$ .
Now $H = E + P V$
$∵ Δ H = Δ E + Δ (P V)$
$∴ Δ H = Δ E + Δ (n RT)$
Thus if $Δ T = 0., Δ H = Δ E$
i.e., remain unaffected