Which of the following statements is correct for the spontaneous adsorption of a gas?

For the reaction $\newline X_2O_4 (l) \rightarrow 2XO_2 (g), \newline \Delta U = 2.1$ kcal, $\Delta S = 20$ cal K$^{-1}$ at $300 K.$ Hence, $\Delta G$ is

Which of the following statements is correct for a reversible process in a state of equilibrium?

Which one of the following characteristics is associated with adsorption?

For a given reaction $\Delta H = 35.5$ kJ mol$^{-1}$ and $\Delta S = 83.6$ JK$^{-1}$ mol$^{-1}.$The reaction is spontaneous at (Assume that $\Delta H$ and $\Delta S$ do not vary with temperature)

A gas is allowed to expand in a well-insulated container against a constant external pressure of $2.5$ atm from an initial volume of $2.50$ L to a final volume of $4.50$ L. The change in internal energy $\Delta U$ of the gas in joules will be

The bond dissociation energies of $X_2, Y_2$ and $XY$ are in the ratio of $1:0.5:1.$ If $\Delta H$ for the formation of $XY$ is $-200$ kJ mol$^{-1},$ the bond dissociation energy of $X_2$ will be

The correction factor $a$ to the ideal gas equation corresponds to

Under isothermal condition, a gas at $300$ K expands from $0.1$ L to $0.25$ L against a constant external pressure of $2$ bar. The work done by the gas is$\\$(Given that $1$ L bar $= 100$ J)

In which case change in entropy is negative?

Hydrolysis of sucrose is given by the following reaction:$\\$Sucrose$+ H_2O \rightleftharpoons$Glucose$+$Fructose$\\$If the equilibrium constant $K_c$ is $2 \times 10^{13}$ at 300 K, the value of $\Delta_r G^0$ at the same temperature will be:

For the reaction, $2$Cl$(g) \rightarrow$Cl$_2(g),$ the correct option is:

The correct option for free expansion of an ideal gas under adiabatic condition is:

Which one among the following is the correct option for the right relationship between$C_P$ and $C_V$ for one mole of an ideal gas?

The maximum temperature that can be achieved in a blast furnace is:

For a reaction $A \to B,$ enthalpy of reaction is $-4.2$ kJ mol$^{-1}$ and enthalpy of activation is $9.6$ kJ mol$^{-1}.$ The correct potential energy profile for the reaction is shown in option.

For irreversible expansion of an ideal gas under isothermal condition, the correct option is:

Which of the following p-V curves represents maximum work done?

Assertion A: In equation $\Delta_r G = - nF E_{cell},$ value of $\Delta_r G$ depends on n.$\\$Reason R: $E_{cell}$ is an intensive property and $\Delta_r G$ is an extensive property.

Which amongst the following options is the correct relation between change in enthalpy and change in internal energy?

$\newline$Match List I with List II

Which of the following processes entropy increases? $\newline$ A. A liquid evaporates to vapour. $\newline$ B. Temperature of a crystalline solid lowered from 130 K to 0 K. $\newline$ C. $2$ NaHCO$_3(s) \rightarrow$ Na$_2$CO$_3(s) +$ CO$_2(g) +$ H$_2$O(g)$\newline$ D. $$ Cl$_2(g) \rightarrow 2$ Cl(g)