MHT CET 2025 23rd April Evening Shift | Thermodynamics Question 1 | Chemistry

i. $\quad 2 \mathrm{H}_{2(\mathrm{~g})}+\mathrm{N}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_2 \mathrm{H}_{4(\mathrm{~g})} ; \Delta_{\mathrm{r}} \mathrm{H}_1^0=95.4 \mathrm{~kJ}$

ii. $\quad \mathrm{N}_2 \mathrm{H}_{4(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}$;$$ \Delta_{\mathrm{t}} \mathrm{H}_2^0=-187.6 \mathrm{~kJ} $$

-92.2 kJ

-46.1 kJ

-138.3 kJ

-283.2 kJ

MHT CET 2025 23rd April Evening Shift

MCQ (Single Correct Answer)

-0

Identify from following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.

$\Delta \mathrm{H}<0$ and $\Delta \mathrm{S}<0$

$\Delta \mathrm{H}>0$ and $\Delta \mathrm{S}>0$

$\Delta \mathrm{H}<0$ and $\Delta \mathrm{S}>0$

$\Delta \mathrm{H}>0$ and $\Delta \mathrm{S}<0$

MHT CET 2025 23rd April Evening Shift

MCQ (Single Correct Answer)

-0

Calculate work done if 1 mole of an ideal gas expands isothermally from $2 \mathrm{dm}^3$ to $2.8 \mathrm{dm}^3$ against constant external pressure 1 atm .

-40.52 J

$\quad-81.04 \mathrm{~J}$

-121.56 J

-60.78 J

MHT CET 2025 23rd April Morning Shift

MCQ (Single Correct Answer)

-0

Which from following reactions is exothermic?

$\mathrm{KOH}_{(\mathrm{aq})}+\mathrm{HNO}_{3(\mathrm{aq})} \longrightarrow \mathrm{KNO}_{3(\mathrm{aq})}+\mathrm{H}_2 \mathrm{O}$

$\mathrm{H}_2 \mathrm{O}_{(\mathrm{s})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(l)}$

$\mathrm{NaCl}_{(\mathrm{s})}+\mathrm{aq} \longrightarrow \mathrm{Na}_{(\mathrm{aq})}^{+}+\mathrm{Cl}_{(\mathrm{aq})}^{-}$

$\mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NO}_{2(\mathrm{~g})}$

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