JEE Main 2012 — Physical Chemistry

A transition metal $M$ forms a volatile chloride which has a vapour density of $94.8$. If it contains $74.75 \%$ of chlorine the formula of the metal chloride will be

An aqueous solution of oxalic acid dihydrate contains its $6.3 \mathrm{~g}$ in $250 \mathrm{ml}$. The volume of $0.1 \mathrm{~N}$ $\mathrm{NaOH}$ required to completely neutralize $10 \mathrm{ml}$ of this solution

$K_1, K_2$ and $K_3$ are the equilibrium constants of the following reactions (I), (II) and (III) respectively: (I) $\mathrm{N}_2+2 \mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}_2$ (II) $2 \mathrm{NO}_2 \rightleftharpoons \mathrm{N}_2+2 \mathrm{O}_2$ (III) $\mathrm{NO}_2 \rightleftharpoons \frac{1}{2} \mathrm{~N}_2+\mathrm{O}_2$ The correct relation from the following is

For a first order reaction, $(A) \rightarrow$ products, the concentration of $A$ changes from $0.1 \mathrm{~M}$ to $0.025 \mathrm{~M}$ in $40$ minutes. The rate of reaction when the concentration of $A$ is $0.01 \mathrm{~M}$ is :

For a reaction $A \rightarrow$ Products, a plot of $\log t_{1 / 2}$ versus $\log a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0$, the order of the reaction is 

$\mathrm{K}_{\mathrm{f}}$ for water is $1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. If your automobile radiator holds $1.0 \mathrm{~kg}$ of water, how many grams of ethylene glycol $\left(\mathrm{C}_2 \mathrm{H}_6 \mathrm{O}_2\right)$ must you add to get the freezing point of the solution lowered to $-2.8^{\circ} \mathrm{C}$ ?

Given (i) $\operatorname{HCN}(a q)+\mathrm{H}_2 \mathrm{O}(b) \rightleftharpoons \mathrm{H}_3 \mathrm{O}^{+}(a q)+\mathrm{CN}^{-}(a q)$ $K_{\mathrm{a}}=6.2 \times 10^{-10}$ (ii) $\mathrm{CN}^{-}(a q)+\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)$ $K_{\mathrm{b}}=1.6 \times 10^{-5}$. These equilibria show the following order of the relative base strength,

Given $$ \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\circ}=0.34 \mathrm{~V}, \mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\circ}=0.15 \mathrm{~V} $$ Standard electrode potential for the half cell $\mathrm{Cu}^{+} / \mathrm{Cu}$ is

If $K_{s p}$ of $\mathrm{CaF}_2$ at $25^{\circ} \mathrm{C}$ is $1.7 \times 10^{-10}$, the combination amongst the following which gives a precipitate of $\mathrm{CaF}_2$ is

If the kinetic energy of an electron is increased four times, the wavelength of the de-Broglie wave associated with it would become

If the radius of first orbit of $\mathrm{H}$ atom is $a_0$, the deBroglie wavelength of an electron in the third orbit is

In a chemical reaction $A$ is converted into $B$. The rates of reaction, starting with initial concentrations of $A$ as $2 \times 10^{-3} \mathrm{M}$ and $1 \times 10^{-3}$ $\mathrm{M}$, are equal to $2.40 \times 10^{-4} \mathrm{Ms}^{-1}$ and $0.60 \times 10^{-4} \mathrm{Ms}^{-1}$ respectively. The order of reaction with respect to reactant $A$ will be

In the following balanced reaction,  values of $X, Y$ and $Z$ respectively are

Liquids A and B form an ideal solution. At $30^{\circ} \mathrm{C}$, the total vapour pressure of a solution containing $1 \mathrm{~mol}$ of A and $2 \mathrm{~mol}$ of B is $250 \mathrm{~mm} \mathrm{Hg}$. The total vapour pressure becomes $300 \mathrm{~mm} \mathrm{Hg}$ when 1 more mol of $\mathrm{A}$ is added to the first solution. The vapour pressures of pure $\mathrm{A}$ and $\mathrm{B}$ at the same temperature are

$8 \mathrm{~mol}$ of $A B_3(\mathrm{~g})$ are introduced into a $1.0 \mathrm{dm}^3$ vessel. If it dissociates as $2 \mathrm{AB}_3(g) \rightleftharpoons A_2(g)+3 B_2(g)$. At equilibrium, $2 \mathrm{~mol}$ of $A_2$ are found to be present. The equilibrium constant of this reaction is

$5 \mathrm{~g}$ of benzene on nitration gave $6.6 \mathrm{~g}$ of nitrobenzene. The theoretical yield of the nitrobenzene will be

One mole of an ideal gas is expanded isothermally and reversibly to half of its initial pressure. $\Delta S$ for the process in $\mathrm{J} \mathrm{K}^{-1} \mathrm{~mol}^{-1}$ is $[\ln 2=0.693$ and $R=8.314, \mathrm{~J} /(\mathrm{mol} \mathrm{K})]$

One mole of $\mathrm{O}_{2(\mathrm{~g})}$ and two moles of $\mathrm{SO}_{2(\mathrm{~g})}$ were heated in a closed vessel of one-litre capacity at $1098 \mathrm{~K}$. At equilibrium $1.6$ moles of $\mathrm{SO}_{3(\mathrm{~g})}$ were found. The equilibrium constant $K_c$ of the reaction would be

Reaction rate between two substance $A$ and $B$ is expressed as following: rate $=k[A]^n[B]^m$ If the concentration of $\mathrm{A}$ is doubled and concentration of $\mathrm{B}$ is made half of initial concentration, the ratio of the new rate to the earlier rate will be:

The activation energy for a reaction which doubles the rate when the temperature is raised from $298 \mathrm{~K}$ to $308 \mathrm{~K}$ is

The concentrated sulphuric acid that is peddled commercial is $95 \% \mathrm{H}_2 \mathrm{SO}_4$ by weight. If the density of this commercial acid is $1.834 \mathrm{~g} \mathrm{~cm}^{-3}$, the molarity of this solution is

The density of a solution prepared by dissolving $120 \mathrm{~g}$ of urea (mol. Mass $=60 \mathrm{u}$ ) in $1000 \mathrm{~g}$ of water is $1.15 \mathrm{~g} / \mathrm{mL}$. The molarity of this solution is :

The difference between the reaction enthalpy change $\left(\Delta_{\mathrm{r}} \mathrm{H}\right)$ and reaction internal energy change $\left(\Delta_{\mathrm{r}} \mathrm{U}\right)$ for the reaction: $$ 2 \mathrm{C}_6 \mathrm{H}_6(\mathrm{l})+15 \mathrm{O}_2(\mathrm{~g}) \longrightarrow $$ at $300 \mathrm{~K}$ is $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

The electron affinity of chlorine is $3.7 \mathrm{eV} .1$ gram of chlorine is completely converted to $\mathrm{Cl}^{-}$ion in a gaseous state. $\left(1 \mathrm{eV}=23.06 \mathrm{kcal} \mathrm{mol}^{-1}\right)$. Energy released in the process is

The electrons identified by quantum numbers $\mathrm{n}$ and $\mathrm{I}$ : (a) $n=4, I=1$ (b) $n=4, l=0$ (c) $n=3, I=2$ (d) $n=3, I=1$ Can be placed in order of increasing energy as:

The enthalpy of neutralisation of $\mathrm{NH}_4 \mathrm{OH}$ with $\mathrm{HCl}$ is $-51.46 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and the enthalpy of neutralisation of $\mathrm{NaOH}$ with $\mathrm{HCl}$ is $-55.90 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The enthalpy of ionisation of $\mathrm{NH}_4 \mathrm{OH}$ is

The entropy of a sample of a certain substance increases by $0.836 \mathrm{~J} \mathrm{~K}^{-1}$ on adding reversibly $0.3344 \mathrm{~J}$ of heat at constant temperature. The temperature of the sample is:

The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ for the reaction $\mathrm{N}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NO}(\mathrm{g})$ at temperature $\mathrm{T}$ is $4 \times 10^{-4}$. The value of $\mathrm{K}_{\mathrm{c}}$ for the reaction, $\mathrm{NO}(\mathrm{g}) \rightarrow{1 / 2} \mathrm{~N}_2(\mathrm{g})+{1 / 2} \mathrm{~O}_2(\mathrm{g})$ at the same temperature is :

The following sets of quantum numbers represent four electrons in an atom. (i) $n=4, l=1$ (ii) $n=4, l=0$ (iii) $n=3, l=2$ (iv) $n=3, l=1$ The sequence representing increasing order of energy, is

The freezing point of a $1.00 \mathrm{~m}$ aqueous solution of $\mathrm{HF}$ is found to be $-1.91^{\circ} \mathrm{C}$. The freezing point constant of water, $K_f$ is $1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. The percentage dissociation of $\mathrm{HF}$ at this concentration is

The incorrect expression among the following is :

The increasing order of the ionic radii of the given isoelectronic species is :

The limiting line in Balmer series will have a frequency of (Rydberg constant, $R_{\infty}=3.29 \times 10^{15}$ cycles $/ \mathrm{s}$ )

The pH of a $0.1$ molar solution of the acid $\mathrm{HQ}$ is $3$ . The value of the ionization constant, Ka of this acid is :

The ppm level of $\mathrm{F}^{-}$in a $500 \mathrm{~g}$ sample of a tooth paste containing $0.2 \mathrm{~g} \mathrm{~F}^{-}$is

The ratio of number of oxygen atoms $(\mathrm{O})$ in $16.0 \mathrm{~g}$ ozone $\left(\mathrm{O}_3\right), 28.0 \mathrm{~g}$ carbon monoxide $(\mathrm{CO})$ and $16.0$ oxygen $\left(\mathrm{O}_2\right)$ is (Atomic mass : $\mathrm{C}=12, \mathrm{O}=16$ and Avogadro's constant $\mathrm{N}_{\mathrm{A}}=6.0 \times 10^{23} \mathrm{~mol}^{-1}$ )

The solubility (in mol $\mathrm{L}^{-1}$ ) of $\mathrm{AgCl}$ $\left(K_{\mathrm{sp}}=1.0 \times 10^{-10}\right)$ in a $0.1 \mathrm{M} \mathrm{KCl}$ solution will be

The solubility of $\mathrm{PbI}_2$ at $25^{\circ} \mathrm{C}$ is $0.7 \mathrm{~g} \mathrm{~L}^{-1}$. The solubility product of $\mathrm{PbI}_2$ at this temperature is (molar mass of $\mathrm{PbI}_2=461.2 \mathrm{~g} \mathrm{~mol}^{-1}$ )

The standard potentials of $\mathrm{Ag}^{+} / \mathrm{Ag}, \mathrm{Hg}_2{ }^{2+} / 2 \mathrm{Hg}$, $\mathrm{Cu}^{2+} / \mathrm{Cu}$ and $\mathrm{Mg}^{2+} / \mathrm{Mg}$ electrodes are $0.80,0.79$, $0.34$ and $-2.37 \mathrm{~V}$, respectively. An aqueous solution which contains one mole per litre of the salts of each of the four metals is electrolyzed. With increasing voltage, the correct sequence of deposition of the metals at the cathode is

The standard reduction potentials for $\mathrm{Zn}^{2+} / \mathrm{Zn}, \mathrm{Ni}^{2+} / \mathrm{Ni}$, and $\mathrm{Fe}^{2+} / \mathrm{Fe}$ are $-0.76,-0.23$ and $-0.44 \mathrm{~V}$ respectively. The reaction $\mathrm{X}+\mathrm{Y}^{2+} \rightarrow \mathrm{X}^{2+}+\mathrm{Y}$ will be spontaneous when:

The value of $K_p$ for the equilibrium reaction $\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g)$ is 2 . The percentage dissociation of $\mathrm{N}_2 \mathrm{O}_4(g)$ at a pressure of $0.5 \mathrm{~atm}$ is

When $\mathrm{CO}_{2(\mathrm{~g})}$ is passed over red hot coke it partially gets reduced to $\mathrm{CO}(g)$. Upon passing $0.5 \mathrm{~L}$ of $\mathrm{CO}_2(g)$ over red hot coke, the total volume of the gases increased to $700 \mathrm{~mL}$. The composition of the gaseous mixture at STP is

Which of the following paramagnetic ions would exhibit a magnetic moment (spin only) of the order of $5 \mathrm{BM}$ ? (At. Nos. $\mathrm{Mn}=25, \mathrm{Cr}=24, \mathrm{~V}=23, \mathrm{Ti}=22$ )