NEET UG 2017 — Physical Chemistry

Which one of the following statements is not correct?

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

Concentration of the ${\mathrm{Ag}}^{+}$ ions in a saturated solution of ${\mathrm{Ag}}_{2}{C}_{2}{O}_{4}$ is $2.2\times {10}^{-4} \mathrm{mol} {L}^{-1}.$ Solubility product of ${\mathrm{Ag}}_{2}{C}_{2}{O}_{4}$ is

Which one of the following statements is wrong?

Which of the following is dependent on temperature?

A first-order reaction has a specific reaction rate ${10}^{-2}{\mathrm{sec}}^{-1}⁡.$ How much time will it take for $20g$ the reactant to reduce to $5g$?

Mechanism of a hypothetical reaction ${X}_{2}+{Y}_{2}\rightarrow 2\mathrm{XY}$ is given below: (i) ${X}_{2}\rightarrow X+X (\mathrm{fast})$ (ii) $X+{Y}_{2}\rightleftharpoons \mathrm{XY}+Y(\mathrm{slow})$ (iii) $X+Y\rightarrow \mathrm{XY} (\mathrm{fast})$ The overall order of the reaction will be

In the electrochemical cell: $\mathrm{Zn}|{\mathrm{ZnSO}}_{4}(0.01M)||{\mathrm{CuSO}}_{4}(1.0 M)|\mathrm{Cu},$ the emf of this Daniel cell is ${E}_{1}$ . When the concentration ${\mathrm{ZnSO}}_{4}$ is changed to $1.0M$ and that of ${\mathrm{CuSO}}_{4}$ changed to $0.01M,$ the emf changes to ${E}_{2}$ . From the following, which one is the relationship between ${E}_{1}$ and ${E}_{2}$? (Given, $\frac{\mathrm{RT}}{F}=0.059$)

If molality of the dilute solution is doubled, the value of molal depression constant $({K}_{f})$ will be

For a given reaction, $\text{Δ}\text{H}=35.5 \text{k}\text{J} \text{m}\text{o}{\text{l}}^{-1}$ and $\text{Δ}\text{S}=83.6 \text{J}{\text{K}}^{-1}\text{m}\text{o}{\text{l}}^{-1}.$ The reaction is spontaneous at : (Assume that $\text{Δ}\text{H}$ and $\text{Δ}\text{S}$ do not vary with temperature)

The equilibrium constants of the following are: $\begin{matrix}{N}_{2}+3{H}_{2}\rightleftharpoons 2 {\mathrm{NH}}_{3} & {K}_{1} \\ {N}_{2}+{O}_{2}\rightleftharpoons 2 \mathrm{NO} & {K}_{2} \\ {H}_{2}+\frac{1}{2}{O}_{2}\rightarrow {H}_{2}O & {K}_{3}\end{matrix}$ The equilibrium constant ($K$) of the reaction: $2N⁡H{⁡}_{3}+\frac{5}{2}O{⁡}_{2}\overset{K⁡}{\rightleftharpoons }2N⁡O⁡+3H{⁡}_{2}O⁡$, will be: