MHT CET 2025 26th April Evening Shift | Thermodynamics Question 5 | Chemistry

$$ \begin{aligned} & \mathrm{CH}_{4(\mathrm{~s})}+2 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\ell)} \\ & \text { if } \Delta_{\mathrm{f}} \mathrm{H}^{-}\left(\mathrm{CH}_4\right)=-75 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} $$

$$ \Delta_{\mathrm{f}} \mathrm{H}^*\left(\mathrm{CO}_2\right)=-390 \mathrm{~kJ} \mathrm{~mol}^{-1} $$

$$ \Delta_{\mathrm{r}} \mathrm{H}^{\circ}\left(\mathrm{H}_2 \mathrm{O}\right)=-286 \mathrm{~kJ} \mathrm{~mol}^{-1} $$

$-887.00 \mathrm{~kJ}$

$-1325.00 \mathrm{~kJ}$

-1035.00 kJ

-1770.00 kJ

MHT CET 2025 26th April Evening Shift

MCQ (Single Correct Answer)

-0

Identify from following the correct set of thermodynamic conditions for the reaction to be spontaneous at all 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 26th April Morning Shift

MCQ (Single Correct Answer)

-0

Calculate the change in internal energy of the system if work done by the system is 18 joule and absorbs heat 50 joule in a particular reaction.

20 J

32 J

48 J

68 J

MHT CET 2025 26th April Morning Shift

MCQ (Single Correct Answer)

-0

Identify from following the correct set of thermodynamic conditions for a reaction to be nonspontaneous at all temperatures.

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

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