500 J of energy is transferred as heat to 0.5 mol of Argon gas at 298 K and 1.00 atm. The final temperature and the change in internal energy respectively are: Given: R = 8.3 J K-1 mol-1

A liquid when kept inside a thermally insulated closed vessel at $25^{\circ }\mathrm{C}$ was mechanically stirred from outside. What will be the correct option for the following thermodynamic parameters ?

Match List - I with List - II. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-c3ow{border-color:inherit;text-align:center;vertical-align:top} .tg .tg-7btt{border-color:inherit;font-weight:bold;text-align:center;vertical-align:top} .tg .tg-0pky{border-color:inherit;text-align:left;vertical-align:top} List - I (Partial Derivatives) List - II (Thermodynamic Quantity) (A) ${\left(\frac{\partial \mathrm{G}}{\partial \mathrm{T}}\right)}_{\mathrm{P}}$ (I) Cp (B) ${\left(\frac{\partial \mathrm{H}}{\partial \mathrm{T}}\right)}_{\mathrm{P}}$ (II) $-$S (C) ${\left(\frac{\partial \mathrm{G}}{\partial \mathrm{P}}\right)}_{\mathrm{T}}$ (III) Cv (D) ${\left(\frac{\partial \mathrm{U}}{\partial \mathrm{T}}\right)}_{\mathrm{V}}$ (IV) V Choose the correct answer from the options given below :

An ideal gas undergoes a cyclic transformation starting from the point A and coming back to the same point by tracing the path A→B→C→D→A as shown in the three cases above.Choose the correct option regarding ΔU :

Ice at $-5^{\circ }\mathrm{C}$ is heated to become vapor with temperature of $110^{\circ }\mathrm{C}$ at atmospheric pressure. The entropy change associated with this process can be obtained from

The effect of temperature on spontaneity of reactions are represented as : .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-c3ow{border-color:inherit;text-align:center;vertical-align:top} .tg .tg-7btt{border-color:inherit;font-weight:bold;text-align:center;vertical-align:top} .tg .tg-amwm{font-weight:bold;text-align:center;vertical-align:top} $\Delta$H $\Delta$S Temperature Spontaneity (A) $+$ $-$ any T Non spontaneous (B) $+$ $+$ low T spontaneous (C) $-$ $-$ low T Non spontaneous (D) $-$ $+$ any T spontaneous The incorrect combinations are :

Let us consider an endothermic reaction which is non-spontaneous at the freezing point of water. However, the reaction is spontaneous at boiling point of water. Choose the correct option.

$$\begin{array}{rl}& \mathrm{S}(\mathrm{g})+\frac{3}{2}{\mathrm{O}}_2(\mathrm{g})\to {\mathrm{SO}}_3(\mathrm{g})+2x\mathrm{kcal}\\ & {\mathrm{SO}}_2(\mathrm{g})+\frac{1}{2}{\mathrm{O}}_2(\mathrm{g})\to {\mathrm{SO}}_3(\mathrm{g})+y\mathrm{kcal}\end{array}$$ The heat of formation of ${\mathrm{SO}}_2(\mathrm{g})$ is given by :

Which of the following mixing of 1 M base and 1 M acid leads to the largest increase in temperature?

Ice and water are placed in a closed container at a pressure of 1 atm and temperature 273.15 K . If pressure of the system is increased 2 times, keeping temperature constant, then identify correct observation from following

Two vessels A and B are connected via stopcock. The vessel A is filled with a gas at a certain pressure. The entire assembly is immersed in water and is allowed to come to thermal equilibrium with water. After opening the stopcock the gas from vessel A expands into vessel B and no change in temperature is observed in the thermometer. Which of the following statement is true ?

Total enthalpy change for freezing of 1 mol of water at $10^{\circ }\mathrm{C}$ to ice at $-10^{\circ }\mathrm{C}$ is ________ (Given: ${\Delta }_{\text{fus }}\mathrm{H}=x\mathrm{kJ}/\mathrm{mol}$ $$\begin{array}{rl}& {\mathrm{C}}_{\mathrm{p}}\left[{\mathrm{H}}_2\mathrm{O}(\mathrm{l})\right]=y\mathrm{J}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}\\ & {\mathrm{C}}_{\mathrm{p}}\left[{\mathrm{H}}_2\mathrm{O}(\mathrm{s})\right]=z\mathrm{J}{\mathrm{mol}}^{-1}{\mathrm{K}}^{-1}\end{array}$$

Arrange the following in order of magnitude of work done by the system/on the system at constant temperature. (a) $\left|w_{\text{reversible }}\right|$ for expansion in infinite stages. (b) $\left|w_{\text{irreversible }}\right|$ for expansion in single stage. (c) $\left|{\mathrm{w}}_{\text{reversible }}\right|$ for compression in infinite stages. (d) $\left|w_{\text{irreversible }}\right|$ for compression in single stage. Choose the correct answer from the options given below :

Which of the following graphs correctly represents the variation of thermodynamic properties of Haber's process?

Consider the given data : (a) $\mathrm{HCl}(\mathrm{g})+10{\mathrm{H}}_2\mathrm{O}(\mathrm{l})\to \mathrm{HCl}.10{\mathrm{H}}_2\mathrm{O}\Delta \mathrm{H}=-69.01\mathrm{kJ}{\mathrm{mol}}^{-1}$ (b) $\mathrm{HCl}(\mathrm{g})+40{\mathrm{H}}_2\mathrm{O}(\mathrm{l})\to \mathrm{HCl}.40{\mathrm{H}}_2\mathrm{O}\Delta \mathrm{H}=-72.79\mathrm{kJ}{\mathrm{mol}}^{-1}$ Choose the correct statement :

The hydration energies of $K^{+}$ and $C{l}^{-}$ are $-x$ and $-y$ kJ/mol respectively. If the lattice energy of KCl is $-z$ kJ/mol, then the heat of solution of KCl is :

The correct statement amongst the following is :

One mole of an ideal gas expands isothermally and reversibly from $10{\mathrm{dm}}^3$ to $20{\mathrm{dm}}^3$ at 300 K . $\Delta \mathrm{U},\mathrm{q}$ and work done in the process respectively are Given: $\mathrm{R}=8.3\mathrm{J}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$ $\ln 10=2.3$ $\log 2=0.30$ $$\log 3=0.48$$

Let us consider a reversible reaction at temperature, T. In this reaction, both $\Delta \mathrm{H}$ and $\Delta \mathrm{S}$ were observed to have positive values. If the equilibrium temperature is Te , then the reaction becomes spontaneous at:

Given below are two statements: Statement I : When a system containing ice in equilibrium with water (liquid) is heated, heat is absorbed by the system and there is no change in the temperature of the system until whole ice gets melted. Statement II : At melting point of ice, there is absorption of heat in order to overcome intermolecular forces of attraction within the molecules of water in ice and kinetic energy of molecules is not increased at melting point. In the light of the above statements, choose the correct answer from the options given below