Sample Quiz

For the following reaction \(2 \mathrm{X}+\mathrm{Y} \stackrel{\mathrm{k}}{\longrightarrow} \mathrm{P}\) the rate of reaction is \(\frac{\mathrm{d}[\mathrm{P}]}{\mathrm{dt}}=\mathrm{k}[\mathrm{X}]\). Two moles of \(\mathbf{X}\) are mixed with one mole of \(\mathbf{Y}\) to make \(1.0 \mathrm{~L}\) of solution. At \(50 \mathrm{~s}, 0.5\) mole of \(\mathbf{Y}\) is left in the reaction mixture. The correct statement(s) about the reaction is(are)
(Use: \(\ln 2=0.693\) )

Some standard electrode potentials at \(298 \mathrm{~K}\) are given below:
\(
\begin{aligned}
&\mathrm{Pb}^{2+} / \mathrm{Pb}-0.13 \mathrm{~V} \\
&\mathrm{Ni}^{2+/} \mathrm{Ni}-0.24 \mathrm{~V} \\
&\mathrm{Cd}^{2+} / \mathrm{Cd}-0.40 \mathrm{~V} \\
&\mathrm{Fe}^{2+} / \mathrm{Fe}-0.44 \mathrm{~V}
\end{aligned}
\)
To a solution containing \(0.001 \mathbf{M}\) of \(\mathbf{X}^{2+}\) and \(0.1 \mathbf{M}\) of \(\mathbf{Y}^{2+}\), the metal rods \(\mathbf{X}\) and \(\mathbf{Y}\) are inserted (at \(298 \mathrm{~K}\) ) and connected by a conducting wire. This resulted in dissolution of \(\mathbf{X}\). The correct combination(s) of \(\mathbf{X}\) and \(\mathbf{Y}\), respectively, is(are)
(Given: Gas constant, \(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\),
Faraday constant, \(\mathrm{F}=96500  \mathrm{C} \mathrm{mol}^{-1}\) )

The pair(s) of complexes wherein both exhibit tetrahedral geometry is(are)
(Note: py = pyridine; Given: Atomic numbers of \(\mathrm{Fe}, \mathrm{Co}, \mathrm{Ni}\) and \(\mathrm{Cu}\) are \(26,27,28\) and 29 , respectively)

The correct statement(s) related to oxoacids of phosphorous is(are)

At \(298 \mathrm{~K}\), the limiting molar conductivity of a weak monobasic acid is \(4 \times 10^{2} \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}\). At \(298 \mathrm{~K}\), for an aqueous solution of the acid the degree of dissociation is \(\alpha\) and the molar conductivity is \(\mathrm{y} \times 10^{2} \mathrm{~S} \mathrm{} \mathrm{cm}^{2} \mathrm{~mol}^{-1}\). At \(298 \mathrm{~K}\), upon 20 times dilution with water, the molar conductivity of the solution becomes \(3 \mathrm{y} \times 10^{2} \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}\)

The value of \(\alpha\) is ______.

At \(298 \mathrm{~K}\), the limiting molar conductivity of a weak monobasic acid is \(4 \times 10^{2} \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}\). At \(298 \mathrm{~K}\), for an aqueous solution of the acid the degree of dissociation is \(\alpha\) and the molar conductivity is \(\mathrm{y} \times 10^{2} \mathrm{~S} \mathrm{} \mathrm{cm}^{2} \mathrm{~mol}^{-1}\). At \(298 \mathrm{~K}\), upon 20 times dilution with water, the molar conductivity of the solution becomes \(3 \mathrm{y} \times 10^{2} \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}\)

The value of \(\mathbf{y}\) is ______.

Reaction of \(\mathbf{x}  g\) of Sn with \(\mathrm{HCl}\) quantitatively produced a salt. The entire amount of the salt reacted with \(\mathbf{y}  g\) of nitrobenzene in the presence of required amount of \(\mathrm{HCl}\) to produce \(1.29 \mathrm{~g}\) of an organic salt (quantitatively).
(Use Molar masses (in \( g  \mathrm{mol}^{-1}\) ) of \(\mathrm{H}, \mathrm{C}, \mathrm{N}, \mathrm{O}, \mathrm{Cl}\) and \(\mathrm{Sn}\) as \(1,12,14,16,35\) and 119 , respectively).
The value of \(x\) is ______.

Reaction of \(\mathbf{x}  g\) of Sn with \(\mathrm{HCl}\) quantitatively produced a salt. The entire amount of the salt reacted with \(\mathbf{y}  g\) of nitrobenzene in the presence of required amount of \(\mathrm{HCl}\) to produce \(1.29 \mathrm{~g}\) of an organic salt (quantitatively).
(Use Molar masses (in \( g  \mathrm{mol}^{-1}\) ) of \(\mathrm{H}, \mathrm{C}, \mathrm{N}, \mathrm{O}, \mathrm{Cl}\) and \(\mathrm{Sn}\) as \(1,12,14,16,35\) and 119 , respectively).
The value of \(y\) is ______.

A sample \((5.6 \mathrm{~g})\) containing iron is completely dissolved in cold dilute HCl to prepare a \(250 \mathrm{~mL}\) of solution. Titration of \(25.0 \mathrm{~mL}\) of this solution requires \(12.5 \mathrm{~mL}\) of \(0.03  \mathrm{M}  \mathrm{KMO}_{4}\) solution to reach the end point. Number of moles of \(\mathrm{Fe}^{2+}\) present in \(250 \mathrm{~mL}\) solution is \(\mathbf{x} \times 10^{-2}\) (consider complete dissolution of \(\left.\mathrm{FeCl}_{2}\right)\). The amount of iron present in the sample is \(\mathbf{y} \%\) by weight.
(Assume: \(\mathrm{KMnO}_{4}\) reacts only with \(\mathrm{Fe}^{2+}\) in the solution; Use: Molar mass of iron as \(56 \mathrm{~g} \mathrm{~mol}^{-1}\) )
The value of \(\mathbf{x}\) is _____.

A sample \((5.6 \mathrm{~g})\) containing iron is completely dissolved in cold dilute HCl to prepare a \(250 \mathrm{~mL}\) of solution. Titration of \(25.0 \mathrm{~mL}\) of this solution requires \(12.5 \mathrm{~mL}\) of \(0.03  \mathrm{M}  \mathrm{KMO}_{4}\) solution to reach the end point. Number of moles of \(\mathrm{Fe}^{2+}\) present in \(250 \mathrm{~mL}\) solution is \(\mathbf{x} \times 10^{-2}\) (consider complete dissolution of \(\left.\mathrm{FeCl}_{2}\right)\). The amount of iron present in the sample is \(\mathbf{y} \%\) by weight.
(Assume: \(\mathrm{KMnO}_{4}\) reacts only with \(\mathrm{Fe}^{2+}\) in the solution; Use: Molar mass of iron as \(56 \mathrm{~g} \mathrm{~mol}^{-1}\) )
The value of \(\mathbf{y}\) is _____.