(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)

JEE MAIN 2021 All JEE MAIN

A
$12$
B
$125$
C
$82$
D
$74$

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Mix Examples-Thermodynamics and Thermochemistry

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For the following reaction $Fe_2O_{3(s)} + 3 CO_{(g)} \longrightarrow 2 Fe_{(s)} + 3 CO_{2(g)}$,$\Delta H^{\circ} = -29.8 \ kJ$ and $\Delta S^{\circ} = 15 \ JK^{-1}$. What is the value of $\Delta S_{\text{total}}$ at $298 \ K$ (in $JK^{-1}$)?

MediumMHT CET 2020

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If $92 \ g$ of $Na$ reacts with water in an open vessel at $300 \ K$, what is the value of work done (in $J$)? $[$Assume ideal nature of the gaseous product$]$

DifficultTS EAMCET 2022

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Calculate the enthalpy change when $50 \ mL$ of $0.01 \ M$ $Ca(OH)_2$ reacts with $25 \ mL$ of $0.01 \ M$ $HCl$. Given that $\Delta H^o_{\text{neutralisation}}$ of strong acid and strong base is $-57.1 \ kJ \ mol^{-1}$. [Assuming that $Ca(OH)_2$ is a strong base]

Difficult

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$CsOH + HCl \to CsCl + H_2O$,$\Delta H = -13.4 \ K \ cal/mol$
$CsOH + HA \to CsA + H_2O$,$\Delta H = -10.4 \ K \ cal/mol$
Then calculate $\Delta H$ of ionisation of $HA$ in $K \ cal/mol$.

Medium

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$1 \ mol$ of $NH_3$ $(\gamma = 4/3)$ gas at $27 \ ^\circ C$ is expanded under reversible adiabatic conditions to make the volume $8$ times. Calculate the work done in $cal$.

Medium

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For the following reaction $Fe_2O_{3(s)} + 3 CO_{(g)} \longrightarrow 2 Fe_{(s)} + 3 CO_{2(g)}$,$\Delta H^{\circ} = -29.8 \ kJ$ and $\Delta S^{\circ} = 15 \ JK^{-1}$. What is the value of $\Delta S_{\text{total}}$ at $298 \ K$ (in $JK^{-1}$)?

If $92 \ g$ of $Na$ reacts with water in an open vessel at $300 \ K$, what is the value of work done (in $J$)? $[$Assume ideal nature of the gaseous product$]$

Calculate the enthalpy change when $50 \ mL$ of $0.01 \ M$ $Ca(OH)_2$ reacts with $25 \ mL$ of $0.01 \ M$ $HCl$. Given that $\Delta H^o_{\text{neutralisation}}$ of strong acid and strong base is $-57.1 \ kJ \ mol^{-1}$. [Assuming that $Ca(OH)_2$ is a strong base]

$CsOH + HCl \to CsCl + H_2O$,$\Delta H = -13.4 \ K \ cal/mol$$CsOH + HA \to CsA + H_2O$,$\Delta H = -10.4 \ K \ cal/mol$Then calculate $\Delta H$ of ionisation of $HA$ in $K \ cal/mol$.

$1 \ mol$ of $NH_3$ $(\gamma = 4/3)$ gas at $27 \ ^\circ C$ is expanded under reversible adiabatic conditions to make the volume $8$ times. Calculate the work done in $cal$.

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$CsOH + HCl \to CsCl + H_2O$,$\Delta H = -13.4 \ K \ cal/mol$
$CsOH + HA \to CsA + H_2O$,$\Delta H = -10.4 \ K \ cal/mol$
Then calculate $\Delta H$ of ionisation of $HA$ in $K \ cal/mol$.