1 mole of an ideal gas at 25° C is subjected to expand reversibly and adiabatically to ten times of its initial volume. Calculate the change in entropy during expansion (in J k -1 mol -1 )

Question

1 mole of an ideal gas at 25° C is subjected to expand reversibly and adiabatically to ten times of its initial volume. Calculate the change in entropy during expansion (in J k -1 mol -1 ) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Δ S=n Cv ln (T2/T1)+n R ln (V2/V1) For adiabatic process (Q=0) Δ E = W n C v ln ( T 2/ T 1)=- nR ln ( V 2/ V 1) ∴ Δ S =0

Q. $1$ mole of an ideal gas at $2 5^{\circ} C$ is subjected to expand reversibly and adiabatically to ten times of its initial volume. Calculate the change in entropy during expansion (in $J k^{- 1} m o l^{- 1}$ )

$Δ S = n C_{v} ln \frac{T _{2}}{T _{1}} + n R ln \frac{V _{2}}{V _{1}}$
For adiabatic process $(Q = 0)$
$Δ E = W$
$n C_{v} ln \frac{T _{2}}{T _{1}} = - n R ln \frac{V _{2}}{V _{1}}$
$∴ Δ S = 0$

Q. 1 mole of an ideal gas at 25∘C is subjected to expand reversibly and adiabatically to ten times of its initial volume. Calculate the change in entropy during expansion (in Jk−1mol−1 )

ΔS=nCv​lnT1​T2​​+nRlnV1​V2​​ For adiabatic process (Q=0) ΔE=W nCv​lnT1​T2​​=−nRlnV1​V2​​ ∴ΔS=0

Q. $1$ mole of an ideal gas at $2 5^{\circ} C$ is subjected to expand reversibly and adiabatically to ten times of its initial volume. Calculate the change in entropy during expansion (in $J k^{- 1} m o l^{- 1}$ )

$Δ S = n C_{v} ln \frac{T _{2}}{T _{1}} + n R ln \frac{V _{2}}{V _{1}}$
For adiabatic process $(Q = 0)$
$Δ E = W$
$n C_{v} ln \frac{T _{2}}{T _{1}} = - n R ln \frac{V _{2}}{V _{1}}$
$∴ Δ S = 0$