Direct conversion of A to B is difficult,so i | vedclass

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Question

(B) Entropy is a state function, so the change in entropy depends only on the initial and final states, not on the path taken.
For the process $A \ri

Vedclass · Accepted Answer

$+60 \ e.u.$

Vedclass · Answer

(B) Entropy is a state function, so the change in entropy depends only on the initial and final states, not on the path taken.
For the process $A ightarrow B$, we can write the path as $A ightarrow C ightarrow D ightarrow B$.
Therefore, $\Delta S_{(A ightarrow B)} = \Delta S_{(A ightarrow C)} + \Delta S_{(C ightarrow D)} + \Delta S_{(D ightarrow B)}$.
Since $\Delta S_{(D ightarrow B)} = -\Delta S_{(B ightarrow D)}$, we have:
$\Delta S_{(A ightarrow B)} = \Delta S_{(A ightarrow C)} + \Delta S_{(C ightarrow D)} - \Delta S_{(B ightarrow D)}$
Substituting the given values:
$\Delta S_{(A ightarrow B)} = 50 + 30 - 20 = 60 	ext{ e.u.}$

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Similar Questions

Among the following processes,for which process is the change in entropy $(\Delta S)$ negative?

Which of the following statements is correct?

One mole of ice is converted into water at $273 \, K$. The entropy of $H_2O_{(s)}$ and $H_2O_{(l)}$ are $38.20 \, J \, mol^{-1} \, K^{-1}$ and $60.01 \, J \, mol^{-1} \, K^{-1}$ respectively. The enthalpy change for the conversion is $....... \, J \, mol^{-1}$.

Which of the following statements is correct?

$STATEMENT-1:$ There is a natural asymmetry between converting work to heat and converting heat to work.$STATEMENT-2:$ No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.

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$STATEMENT-1:$ There is a natural asymmetry between converting work to heat and converting heat to work.
$STATEMENT-2:$ No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.