JEE Main 2006 — Physical Chemistry

Given the data at $25^{\circ} \mathrm{C}$, $$ \begin{aligned} & \mathrm{Ag}+\mathrm{I}^{-} \longrightarrow \mathrm{AgI}+\mathrm{e}^{-} ; \mathrm{E}^{\circ}=0.152 \mathrm{~V} \\ & \mathrm{Ag} \longrightarrow \mathrm{Ag}^{+}+\mathrm{e}^{-} ; \quad \mathrm{E}^{\circ}=-0.800 \mathrm{~V} \end{aligned} $$ What is the value of $\log \mathrm{K}_{\mathrm{sp}}$ for $\mathrm{AgI}$ ? $$ \left(2.303 \frac{R T}{F}=0.059 \mathrm{~V}\right) $$

How many moles of magnesium phosphate, $\mathrm{Mg}_3\left(\mathrm{PO}_4\right)_2$ will contain $0.25$ mole of oxygen atoms?

According to Bohr's theory, the angular momentum of an electron in $5^{\text {th }}$ orbit is

A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will

$18 \mathrm{~g}$ of glucose $\left(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6\right)$ is added to $178.2 \mathrm{~g}$ of water. The vapour pressure of water for this aqueous solution at $100^{\circ} \mathrm{C}$ is

The enthalpy changes for the following processes are listed below: $\begin{array}{ll}\mathrm{Cl}_2(\mathrm{~g})=2 \mathrm{Cl}(\mathrm{g}), & 242.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_2(\mathrm{~g})=2 \mathrm{I}(\mathrm{g}), & 151.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{ICl}(\mathrm{g})=\mathrm{I}(\mathrm{g})+\mathrm{Cl}(\mathrm{g}), & 211.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_2(\mathrm{~s})=\mathrm{I}_2(\mathrm{~g}), & 62.76 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array}$ Given that the standard states for iodine and chlorine are $\mathrm{I}_2(\mathrm{~s})$ and $\mathrm{Cl}_2(\mathrm{~g})$, the standard enthalpy of formation for $\mathrm{ICl}(\mathrm{g})$ is

The equilibrium constant for the reaction $$ \mathrm{SO}_3(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) $$ is $\mathrm{K}_{\mathrm{c}}=4.9 \times 10^{-2}$. The value of $\mathrm{K}_{\mathrm{c}}$ for the reaction $$ 2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_3(\mathrm{~g}) $$ will be

In the transformation of ${ }_{92}^{238} \mathrm{U}$ to ${ }_{92}^{234} \mathrm{U}$, if one emission is an $\alpha$-particle, what should be the other emission(s)?

$(\Delta \mathrm{H}-\Delta \mathrm{U})$ for the formation of carbon monoxide (CO) from its elements at $298 \mathrm{~K}$ is $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

Rate of a reaction can be expressed by Arrhenius equation as: $$ \mathrm{k}=\mathrm{Ae}^{-\mathrm{E} / \mathrm{RT}} $$ In this equation, E represents

Which of the following statements is true?

The "spin-only" magnetic moment [in units of Bohr magneton, $\left.\left(\mu_{\mathrm{B}}\right)\right]$ of $\mathrm{Ni}^{2+}$ in aqueous solution would be (Atomic number of $\mathrm{Ni}=28$ )

The standard enthalpy of formation $\left(\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\right)$ at $298 \mathrm{~K}$ for methane, $\mathrm{CH}_4(\mathrm{~g})$, is $-74.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The additional information required to determine the average energy for $\mathrm{C}-\mathrm{H}$ bond formation would be

Uncertainty in the position of an electron (mass $=9.1 \times 10^{-31} \mathrm{~kg}$ ) moving with a velocity $300 \mathrm{~ms}^{-1}$, accurate upto $0.001 \%$, will be

An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If $T_i$ is the initial temperature and $T_f$ is the final temperature, which of the following statements is correct?

The following mechanism has been proposed for the reaction of $\mathrm{NO}$ with $\mathrm{Br}_2$ to form $\mathrm{NOBr}$ : $\mathrm{NO}(\mathrm{g})+\mathrm{Br}_2(\mathrm{~g}) \rightleftharpoons \mathrm{NOBr}_2(\mathrm{~g})$ $$ \mathrm{NOBr}_2(\mathrm{~g})+\mathrm{NO}(\mathrm{g}) \longrightarrow 2 \mathrm{NOBr}(\mathrm{g}) $$ If the second step is the rate determining step, the order of the reaction with respect to $N O(g)$ is

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration $0.1 \mathrm{M}$ is $100 \Omega$. The conductivity of this solution is $1.29 \mathrm{~S} \mathrm{~m}^{-1}$. Resistance of the same cell when filled with $0.2 \mathrm{M}$ of the same solution is $520 \Omega$. The molar conductivity of $0.02 \mathrm{M}$ solution of the electrolyte will be

Density of a $2.05 \mathrm{M}$ solution of acetic acid in water is $1.02 \mathrm{~g} / \mathrm{mL}$. The molality of the solution is

Which one of the following sets of ions represents a collection of isoelectronic species?

The molar conductivities $\wedge_{\mathrm{NaOAC}}^{\circ}$ and $\wedge_{\mathrm{HCl}}^{\circ}$ at infinite dilution in water at $25^{\circ} \mathrm{C}$ are $91.0$ and $426.2 \mathrm{~S} \mathrm{~cm}^2 / \mathrm{mol}$ respectively. To calculate $\wedge_{\mathrm{HOAc}}^O$, the additional value required is