(C) $\text{Millimoles of } HCl = 200 \times 0.2 = 40 \ mmol$$\text{Millimoles of } NaOH = 300 \times 0.1 = 30 \ mmol$$\text{Since } NaOH \text{ is the

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(C) $\text{Millimoles of } HCl = 200 \times 0.2 = 40 \ mmol$$\text{Millimoles of } NaOH = 300 \times 0.1 = 30 \ mmol$$\text{Since } NaOH \text{ is the limiting reagent, heat released } (q) = \frac{30}{1000} \times 57.1 \times 1000 = 1713 \ J$$\text{Total mass of solution } (m) = (200 + 300) \ mL \times 1 \ g \ mL^{-1} = 500 \ g$$\Delta T = \frac{q}{m \times C} = \frac{1713}{500 \times 4.18} = \frac{1713}{2090} \approx 0.8196 \ K$$\Delta T = 81.96 \times 10^{-2} \ K$$\text{Since } \Delta T \text{ in } K \text{ is equal to } \Delta T \text{ in } ^{\circ}C, \text{ we have } x = 81.96 \approx 82$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Easy

$200 \ mL$ of $0.2 \ M \ HCl$ is mixed with $300 \ mL$ of $0.1 \ M \ NaOH$. The molar heat of neutralization of this reaction is $-57.1 \ kJ \ mol^{-1}$. The increase in temperature in $^{\circ}C$ of the system on mixing is $x \times 10^{-2}$. The value of $x$ is ....... . (Nearest integer)
[Given : Specific heat of water $= 4.18 \ J \ g^{-1} \ K^{-1}$
Density of water $= 1.00 \ g \ cm^{-3}$]
(Assume no volume change on mixing)

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$12$
B
$125$
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$82$
D
$74$

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For the reaction $2Cl_{(g)} \rightarrow Cl_{2(g)}$,the signs of $\Delta H$ and $\Delta S$ are respectively:

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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

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Standard entropies of $X_2$,$Y_2$ and $XY_3$ are $60$,$40$ and $50 \ J \ K^{-1} \ mol^{-1}$ respectively. For the reaction $\frac{1}{2} X_2 + \frac{3}{2} Y_2 \rightarrow XY_3$,the enthalpy change is $\Delta H = -30 \ kJ \ mol^{-1}$. At what temperature will the reaction be at equilibrium (in $K$)?

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The internal energy change (in $J$) when $90 \ g$ of water undergoes complete evaporation at $100^{\circ} C$ is........
(Given: $\Delta H_{vap}$ for water at $373 \ K = 41 \ kJ/mol$,$R = 8.314 \ J \ K^{-1} mol^{-1}$)