MHT CET 2024 4th May Morning Shift | Thermodynamics Question 34 | Chemistry

Calculate the entropy change for melting 1 g ice at $0^{\circ} \mathrm{C}$ in $\mathrm{Jg}^{-1} \mathrm{~K}^{-1}$ if heat of fusion of ice at $0^{\circ} \mathrm{C}$ is $80 \mathrm{~J} \mathrm{~K}^{-1}$.

0.039

0.293

8.0

27.3

MHT CET 2024 4th May Morning Shift

MCQ (Single Correct Answer)

-0

Which of the following set of properties is correct when one mole of a gas is heated keeping volume constant by increasing temperature and supplying 500 J of heat?

$\mathrm{q}=\mathrm{w}=500 \mathrm{~J}, \Delta \mathrm{U}=0$

$\mathrm{q}=\Delta \mathrm{U}=500 \mathrm{~J}, \mathrm{w}=0$

$\mathrm{q}=\Delta \mathrm{U}=-500 \mathrm{~J}, \mathrm{w}=0$

$\mathrm{q}=500 \mathrm{~J}, \Delta \mathrm{U}=\mathrm{w}=0$

MHT CET 2024 3rd May Evening Shift

MCQ (Single Correct Answer)

-0

Find value of Q from following equations.

(i) $\mathrm{C}_{(\mathrm{s})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{CO}_{2(\mathrm{~g})} \Delta \mathrm{H}=\mathrm{QkJ}$

(ii) $\mathrm{C}_{(\mathrm{s})}+\frac{1}{2} \mathrm{O}_{2(8)} \longrightarrow \mathrm{CO}_{2(8)} \Delta \mathrm{H}=-\mathrm{x} \mathrm{kJ}$

(iii) $\mathrm{C}_{(\mathrm{s})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~s})} \longrightarrow \mathrm{CO}_{2(\mathrm{~g})} \Delta \mathrm{H}=-\mathrm{ykJ}$

$\mathrm{-(x+y) k J}$

$(\mathrm{x}-\mathrm{y}) \mathrm{kJ}$

$\frac{-\mathrm{x}+\mathrm{y}}{2} \mathrm{~kJ}$

$\frac{\mathrm{x}+\mathrm{y}}{2} \mathrm{~kJ}$

MHT CET 2024 3rd May Evening Shift

MCQ (Single Correct Answer)

-0

Which of the following statements is appropriate as per first law of thermodynamics?

Energy of the system remains constant.

Energy of the surrounding remains constant.

Entropy of the universe remains constant.

Energy of the universe remains constant.

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