(D) The change in entropy is given by the formula $\Delta S = \frac{q_{rev}}{T}$.Given,$\Delta S = 0.836 \ J \ K^{-1}$ and $q_{rev} = 0.3344 \ J$.Rear

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(D) The change in entropy is given by the formula $\Delta S = \frac{q_{rev}}{T}$.Given,$\Delta S = 0.836 \ J \ K^{-1}$ and $q_{rev} = 0.3344 \ J$.Rearranging the formula to solve for temperature $T$: $T = \frac{q_{rev}}{\Delta S}$.Substituting the values: $T = \frac{0.3344}{0.836} = 0.4 \ K$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

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The entropy of a sample of a certain substance increases by $0.836 \ J \ K^{-1}$ on adding reversibly $0.3344 \ J$ of heat at constant temperature. The temperature of the sample is.....$K$

AIEEE 2012 All AIEEE

A
$2.5$
B
$0.3$
C
$0.016$
D
$0.4$

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2 nd Law of thermodynamics and Entropy

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The entropy of a sample of a certain substance increases by $0.836 \ J \ K^{-1}$ on adding reversibly $0.3344 \ J$ of heat at constant temperature. The temperature of the sample is.....$K$

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The entropy change involved in the isothermal reversible expansion of $2 \, \text{mole}$ of an ideal gas from a volume of $10 \, dm^3$ to a volume of $100 \, dm^3$ at $27 \, ^oC$ is : .............. $J \, K^{-1}$

What happens to the entropy during the melting of ice to water?

When $2 \ mol$ of an ideal gas $\left( C_{p,m} = \frac{5}{2} R \right)$ is heated from $300 \ K$ to $600 \ K$ at constant pressure,the change in entropy of the gas $\left( \Delta S \right)$ is:

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