Thermodynamics · Chemistry · MHT CET (Biology)

One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at 300 K . Find $\Delta \mathrm{U}, \mathrm{q}$ and work done respectively in the process. $\left(\mathrm{R}=8.3 \times 10^{-3} \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

Calculate heat of formation of $\mathrm{SO}_2$ from following equations.

$$ \begin{aligned} & \mathrm{S}+\frac{3}{2} \mathrm{O}_2 \longrightarrow \mathrm{SO}_3, \Delta \mathrm{H}=-2 \mathrm{xkJ} \\ & \mathrm{SO}_2+\frac{1}{2} \mathrm{O}_2 \longrightarrow \mathrm{SO}_3, \Delta \mathrm{H}=-\mathrm{ykJ} \end{aligned} $$

Which of the following symbols represents heat of reaction at constant pressure?

The entropy of vaporisation of benzene is $85 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$. When 117 g of benzene vaporises at its boiling point, what is entropy change of surrounding if process is at equilibrium?

Which from following terms is explained by first law of thermodynamics?

What is the change in internal energy for $2 \mathrm{CO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}$ at $25^{\circ} \mathrm{C}$ ?

( $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \Delta \mathrm{H}=-560 \mathrm{~kJ}$ )