(A) The entropy change of the surroundings is given by $\Delta S_{surr} = \frac{-\Delta H}{T}$. Given $\Delta H = 28.1 \ kJ \ mol^{-1} = 28100 \ J \

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(A) The entropy change of the surroundings is given by $\Delta S_{surr} = \frac{-\Delta H}{T}$. Given $\Delta H = 28.1 \ kJ \ mol^{-1} = 28100 \ J \ mol^{-1}$ and $T = 300 \ K$. $\Delta S_{surr} = \frac{-28100 \ J \ mol^{-1}}{300 \ K} = -93.67 \ J \ K^{-1} \ mol^{-1}$. The total entropy change is $\Delta S_{total} = \Delta S_{sys} + \Delta S_{surr}$. $\Delta S_{total} = 108.7 \ J \ K^{-1} \ mol^{-1} + (-93.67 \ J \ K^{-1} \ mol^{-1}) = 15.03 \ J \ K^{-1} \ mol^{-1}$. Rounding to one decimal place,we get $15.1 \ J \ K^{-1} \ mol^{-1}$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

Calculate $\Delta S_{total}$ for the following reaction at $300 \ K$.
$NH_4NO_{3(s)} \longrightarrow NH_4^+{(aq)} + NO_3^-{(aq)}$ $(\Delta H = 28.1 \ kJ \ mol^{-1}, \Delta S_{sys} = 108.7 \ J \ K^{-1} \ mol^{-1})$

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A
$15.1 \ J \ K^{-1} \ mol^{-1}$
B
$93.6 \ J \ K^{-1} \ mol^{-1}$
C
$84.3 \ J \ K^{-1} \ mol^{-1}$
D
$202.3 \ J \ K^{-1} \ mol^{-1}$

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Calculate $\Delta S_{total}$ for the following reaction at $300 \ K$. $NH_4NO_{3(s)} \longrightarrow NH_4^+{(aq)} + NO_3^-{(aq)}$ $(\Delta H = 28.1 \ kJ \ mol^{-1}, \Delta S_{sys} = 108.7 \ J \ K^{-1} \ mol^{-1})$

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$9.0 \ g$ of $H_2O$ is vaporised at $100 \ ^oC$ and $1 \ atm$ pressure. If the latent heat of vaporisation of water is $x \ J/g$,then $\Delta S$ is given by

For the reaction $Br_{2(l)} + Cl_{2(g)} \rightarrow 2BrCl_{(g)}$,the enthalpy change is $\Delta H = 30 \ kJ/mol$ and the entropy change is $\Delta S = 105 \ J/mol \cdot K$. The temperature at equilibrium is $...... \ K$.

An isolated box,equally partitioned,contains two ideal gases $A$ and $B$ as shown in the figure. When the partition is removed,the gases mix. The changes in enthalpy $(\Delta H)$ and entropy $(\Delta S)$ in the process,respectively,are

From the following data,the enthalpy of dilution of $KCl$ will be ............ $kJ$.$KCl_{(s)} + 20H_2O \to KCl(20H_2O); \Delta H = + 15.90 \ kJ$$KCl_{(s)} + 200H_2O \to KCl(200H_2O); \Delta H = + 18.58 \ kJ$

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Calculate $\Delta S_{total}$ for the following reaction at $300 \ K$.
$NH_4NO_{3(s)} \longrightarrow NH_4^+{(aq)} + NO_3^-{(aq)}$ $(\Delta H = 28.1 \ kJ \ mol^{-1}, \Delta S_{sys} = 108.7 \ J \ K^{-1} \ mol^{-1})$

From the following data,the enthalpy of dilution of $KCl$ will be ............ $kJ$.
$KCl_{(s)} + 20H_2O \to KCl(20H_2O); \Delta H = + 15.90 \ kJ$
$KCl_{(s)} + 200H_2O \to KCl(200H_2O); \Delta H = + 18.58 \ kJ$