The standard enthalpy of neutralization is $$-57.3 \mathrm{~K}{\mathrm{J}}~ \mathrm{mol}^{-1}$$as:
$$\small{\underset{\text{strong acid}}{\mathrm{HCl_{(aq)}}}+\underset{\text{strong base}}{\mathrm{NaOH_{(aq)}}}\rightarrow\mathrm{NaCl_{(aq)}+H_2O(l),\Delta H=-57.3~KJ mol^{-1}}}$$
The enthalpy of neutralization of $$0.25 \mathrm{~mol}$$ of HCI by $$0.25 \mathrm{~mol}$$ of $$\mathrm{NaOH}$$ is :

1. $$-57.3~ \mathrm{kJ} ~\mathrm{mol}^{-1}$$
2. $$-28.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$$
3. $$-14.32 \mathrm{~kJ} \mathrm{~mol}^{-1}$$
4. $$+57.3~ \mathrm{kJ}~ \mathrm{mol}^{-1}$$
Subtopic:  Thermochemistry |
62%
NEET - 2024
Hints

Consider the following reaction:
$$\mathrm{2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \Delta_rH^\circ = -483.64 kJ. }$$
What is the enthalpy change for the decomposition of one mole of water?
1. 120.9 kJ
2. 241.82 kJ
3. 18 kJ
4. 100 kJ
Subtopic:  Thermochemistry |
86%
From NCERT
NEET - 2023
Hints

At standard conditions, if the change in the enthalpy for the following reaction is –109 kJ mol
H2(g)+Br2(g)$\to$2HBr(g) and the bond energy of H2 and Br2 is 435 kJ mol–1 and 192 kJ mol–1 respectively, what is the bond energy (in kJ mol–1) of HBr?

 1 368 2 736 3 518 4 259
Subtopic:  Thermochemistry |
53%
From NCERT
NEET - 2020
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NEET 2025 - Target Batch
Hints