(C) For the fusion process at the melting point,the relationship between enthalpy of fusion,entropy of fusion,and melting temperature is given by: $\D

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(C) For the fusion process at the melting point,the relationship between enthalpy of fusion,entropy of fusion,and melting temperature is given by: $\Delta_{fus}H = T_{mp} \times \Delta_{fus}S$. Given: $\Delta_{fus}H = 600 \ cal \ mol^{-1}$,$\Delta_{fus}S = 2 \ cal \ mol^{-1} \ K^{-1}$,and $T_{mp} = x \ K$. Substituting the values: $600 = x \times 2$. Solving for $x$: $x = 600 / 2 = 300 \ K$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

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Melting point of a solid is $x \ K$ and its latent heat of fusion is $600 \ cal \ mol^{-1}$. The entropy change for fusion of $1 \ mol$ solid is $2 \ cal \ mol^{-1} \ K^{-1}$. The value of $x$ will be......$K$

A
$100$
B
$200$
C
$300$
D
$400$

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Thermodynamics

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2 nd Law of thermodynamics and Entropy

For an endothermic reaction $A \rightarrow B$ to occur spontaneously at a constant temperature $T$,the entropy change $\Delta S$ must be:

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For chemical reactions,the calculation of change in entropy is normally done:

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According to the second law of thermodynamics,which of the following is true for a spontaneous process?

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Why does the entropy of a substance increase with an increase in temperature?

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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 : .............. $J \, K^{-1}$

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Melting point of a solid is $x \ K$ and its latent heat of fusion is $600 \ cal \ mol^{-1}$. The entropy change for fusion of $1 \ mol$ solid is $2 \ cal \ mol^{-1} \ K^{-1}$. The value of $x$ will be......$K$

Similar Questions

For an endothermic reaction $A \rightarrow B$ to occur spontaneously at a constant temperature $T$,the entropy change $\Delta S$ must be:

For chemical reactions,the calculation of change in entropy is normally done:

According to the second law of thermodynamics,which of the following is true for a spontaneous process?

Why does the entropy of a substance increase with an increase in temperature?

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 : .............. $J \, K^{-1}$

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