(A) Entropy $(S)$ is a state function and its value depends on the state of the system,which is defined by variables like temperature $(T)$,pressure $

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Both $\Delta S$ and $S$ are functions of temperature.

(A) Entropy $(S)$ is a state function and its value depends on the state of the system,which is defined by variables like temperature $(T)$,pressure $(P)$,and volume $(V)$.Since $S = f(T, P, V)$,entropy is a function of temperature.Similarly,the change in entropy $(\Delta S = S_2 - S_1)$ also depends on the initial and final states of the system,which are defined by temperature.Therefore,both $S$ and $\Delta S$ are functions of temperature.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

Medium

The true statement amongst the following is

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A
Both $\Delta S$ and $S$ are functions of temperature.
B
$S$ is not a function of temperature but $\Delta S$ is a function of temperature.
C
Both $S$ and $\Delta S$ are not functions of temperature.
D
$S$ is a function of temperature but $\Delta S$ is not a function of temperature.

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Thermodynamics

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2 nd Law of thermodynamics and Entropy

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What will be $\Delta S$ for the reaction: $2A + 3B \to 4C + 5D$ (in $J \ K^{-1}$)?
Given:
$\Delta S_A^o = 100 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_B^o = 120 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_C^o = 200 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_D^o = 150 \ J \ mol^{-1} \ K^{-1}$

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Maximum entropy will be in which of the following?

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For a spontaneous endothermic process at constant pressure,which of the following is true?

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Which functions are required to understand the second law of thermodynamics?

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One mole of ice is converted into water at $1 \ atm$ and $273 \ K$. The entropies of $H_2O_{(s)}$ and $H_2O_{(\ell)}$ are $38.2$ and $60.01 \ J \ mol^{-1} \ K^{-1}$ respectively. The enthalpy change for the conversion is ...... $J \ mol^{-1}$.

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The true statement amongst the following is

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What will be $\Delta S$ for the reaction: $2A + 3B \to 4C + 5D$ (in $J \ K^{-1}$)?Given:$\Delta S_A^o = 100 \ J \ mol^{-1} \ K^{-1}$$\Delta S_B^o = 120 \ J \ mol^{-1} \ K^{-1}$$\Delta S_C^o = 200 \ J \ mol^{-1} \ K^{-1}$$\Delta S_D^o = 150 \ J \ mol^{-1} \ K^{-1}$

Maximum entropy will be in which of the following?

For a spontaneous endothermic process at constant pressure,which of the following is true?

Which functions are required to understand the second law of thermodynamics?

One mole of ice is converted into water at $1 \ atm$ and $273 \ K$. The entropies of $H_2O_{(s)}$ and $H_2O_{(\ell)}$ are $38.2$ and $60.01 \ J \ mol^{-1} \ K^{-1}$ respectively. The enthalpy change for the conversion is ...... $J \ mol^{-1}$.

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What will be $\Delta S$ for the reaction: $2A + 3B \to 4C + 5D$ (in $J \ K^{-1}$)?
Given:
$\Delta S_A^o = 100 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_B^o = 120 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_C^o = 200 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_D^o = 150 \ J \ mol^{-1} \ K^{-1}$