Chapter 1

\(500 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) contains \(6.0 \times 10^{23}\) molecules at STP. How many molecules are present in \(100 \mathrm{~mL}\) of \(\mathrm{CO}_{2}\) at STP? (a) \(6 \times 10^{23}\) (b) \(1.5 \times 10^{23}\) (c) \(1.2 \times 10^{23}\) (d) none of these

In the reaction, \(4 \mathrm{NH}_{3}+5 \mathrm{O}_{2} \longrightarrow 4 \mathrm{NO}+6 \mathrm{H}_{2} \mathrm{O}\), when one mole of ammonia and one mole of oxygen are made to react to completion, then (a) \(1.0 \mathrm{~mol}\) of \(\mathrm{H}_{2} \mathrm{O}\) is produced (b) all the oxygen is consumed (c) \(1.5 \mathrm{~mol}\) of \(\mathrm{NO}\) is formed (d) all the ammonia is consumed

The number of gram molecules of oxygen in \(6.02 \times\) \(10^{24}\) CO molecules is (a) \(10 \mathrm{~g}\) molecules (b) \(5 \mathrm{~g}\) molecules (c) l g molecules (d) \(0.5 \mathrm{~g}\) molecules

The number of oxalic acid molecules in \(100 \mathrm{ml}\) of \(0.02\) N oxalic acid solution is (a) \(6.023 \times 10^{22}\) (b) \(10^{-3}\) (c) \(6.022 \times 10^{20}\) (d) none of these

In the reaction \(4 \mathrm{NH}_{3}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) when \(1 \mathrm{~mol}\) of ammonia and \(1 \mathrm{~mol}\) of \(\mathrm{O}_{2}\) are made to react to completion then (a) \(1.0 \mathrm{~mol}\) of \(\mathrm{H}_{2} \mathrm{O}\) is produced (b) \(1.0 \mathrm{~mol}\) of \(\mathrm{NO}\) will be produced (c) all the ammonia will be consumed (d) all the oxygen will be consumed

What is the volume (in litres) of \(\mathrm{CO}_{2}\) liberated at STP, when \(2.12\) gram of sodium carbonate (mol. \(\mathrm{wt}=106\) ) is treated with excess dilute HCl? (a) \(11.2\) (b) \(2.12\) (c) \(0.448\) (d) \(4.26\)

Percentage of Se in peroxidase anhydrous enzyme is \(0.5 \%\) by weight (at. wt \(=78.4\) ) then minimum molecular weight of peroxidase anhydrous enzymes is (a) \(1.568 \times 10^{3}\) (b) \(1.568 \times 10^{4}\) (c) \(25.68\) (d) \(4.316 \times 10^{4}\)

For the formation of \(3.65 \mathrm{gm}\) of \(\mathrm{HCl}\), what volume of \(\mathrm{H}_{2}\), and \(\mathrm{Cl}_{2}\) are needed at N.T.P? (a) \(1.12 \mathrm{~L}, 1.12 \mathrm{~L}\) (b) \(1.12 \mathrm{~L}, 2.24 \mathrm{~L}\) (c) \(3.65 \mathrm{~L}, 1.83 \mathrm{~L}\) (d) \(1 \mathrm{~L}, 1 \mathrm{~L}\)

The decomposition of a certain mass of \(\mathrm{CaCO}_{3}\) gave \(11.2 \mathrm{dm}^{3}\) of \(\mathrm{CO}_{2}\) gas at STP. The mass of KOH required to completely neutralize the gas is (a) \(56 \mathrm{~g}\) (b) \(28 \mathrm{~g}\) (c) \(42 \mathrm{~g}\) (d) \(20 \mathrm{~g}\)

If 1 mole of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is reacted with 1 mole of \(\mathrm{X}(\mathrm{OH})_{2}\) as: \(\mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{X}(\mathrm{OH})_{2} \longrightarrow \mathrm{XHPO}_{4}+2 \mathrm{H}_{2} \mathrm{O}\) then (a) The equivalent weight of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is \(\frac{98}{3}\). (b) The equivalent weight of base is \(\frac{\text { Molecular mass }}{2}\) (c) 1 mole of \(\mathrm{X}(\mathrm{OH})_{2}\) more is required for complete neutralization of \(\mathrm{XHPO}_{4}\). (d) The resulting solution required 1 mole \(\mathrm{NaOH}\) for complete neutralization.

Which of the following contain the same number of molecules? (a) \(0.1\) mole of \(\mathrm{CO}_{2}\) (b) \(3.2 \mathrm{~g}\) of \(\mathrm{O}_{2}\) (c) \(0.1 \mathrm{~g}\) atom of Helium gas (d) \(11.2 \mathrm{~L}\) of \(\mathrm{SO}_{2}\) at S.T.P

Which of the following statements are true? (a) \(392 \mathrm{~g}\) of ferrous ammonium sulphate is required to reduce \(31.6 \mathrm{~g} \mathrm{KMnO}_{4}\) in aqueous acidic medium. (b) Molality of a solution does not vary with temperature. (c) \(\mathrm{KBrO}_{3}\) can quantitatively convert \(\mathrm{Br}^{-}\)to \(\mathrm{Br}_{2}\). (d) The oxidation state of \(\mathrm{S}\) in \(\mathrm{CNS}^{-}\)is zero.

Which of the following statement is/are correct? (a) \(\mathrm{CrI}_{3}+\mathrm{KOH}+\mathrm{Cl}_{2} \rightarrow \mathrm{K}_{2} \mathrm{CrO}_{4}+\mathrm{KCl}+\mathrm{KIO}_{4}+\mathrm{H}_{2} \mathrm{O}\) So, in balanced chemical reaction coefficient of \(\mathrm{KOH}\) is 64 . (b) If \(\mathrm{Zn}+\mathrm{KMnO}_{4}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{ZnSO}_{4}+\mathrm{K}_{2} \mathrm{SO}_{4}+\) \(\mathrm{MnSO}_{4}+\mathrm{H}_{2}\); then equivalents of \(\mathrm{Zn}=\) equivalents of \(\mathrm{Zn}=\) equivalents of \(\mathrm{KMnO}_{4}+\) equivalents of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (c) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} \stackrel{\Delta}{\longrightarrow} \mathrm{N}_{2}+\mathrm{Cr}_{2} \mathrm{O}_{3}+\mathrm{H}_{2} \mathrm{O}, \mathrm{n}\)-factor of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) is 12 . (d) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-} \rightarrow \mathrm{Fe}^{3+}+\mathrm{CO}_{2}+\mathrm{NO}_{3}^{-}, \mathrm{n}\)-factor for \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) is \(60 .\)

\(100 \mathrm{ml}\) of \(0.06 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) is added to \(50 \mathrm{~mL}\) of \(0.06\) \(\mathrm{M} \mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4} .\) After the reaction is complete (a) \(0.003 \mathrm{M}\) of excess of \(\mathrm{Ca}^{2+}\) will remain in excess. (b) \(0.003\) moles of calcium oxalate will get precipitated (c) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) is excess reagent. (d) \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) is limiting reagent.

Which of the following contains same number of molecules? (a) \(3.2 \mathrm{~g}\) of \(\mathrm{O}_{2}\) (b) \(0.1\) mole of \(\mathrm{NO}_{2}\) (c) \(0.1 \mathrm{~g}\) atom of Ar gas (d) \(11.2 \mathrm{~L}\) of \(\mathrm{CO}_{2}\) at S.T.P.

What is the \(\%\) of free \(\mathrm{SO}_{3}\) is an oleum that is labeled as \({ }^{4} 104.5 \% \mathrm{H}_{2} \mathrm{SO}_{4}{\underline{\phantom{xx}}}^{\prime} ?\) (a) 30 (b) 10 (c) 20 (d) 40

Match the following $$ \begin{array}{ll} \hline \text { Column-I } & \text { Column-II } \\ \hline \text { (a) } 5.55 \text { mole } & \text { p. } 4.48 \text { litre of } \mathrm{SO}_{2} \text { at NTP } \\ \text { (b) } 0.1 \text { mole } & \text { q. } 100 \mathrm{~mL} \text { of } \mathrm{H}_{2} \mathrm{O} \\ \text { (c) } 0.2 \text { mole } & \text { r. } 22 \mathrm{~g} \text { of } \mathrm{CO}_{2} \\ \text { (d) } 0.5 \text { mole } & \text { s. } 2.24 \text { litre of } \mathrm{NH}_{3} \\ & \text { t. } 0.1 \mathrm{gm} \text { atom of Iron } \\ \hline \end{array} $$

Consider the reaction of \(\mathrm{Br}_{2}\) with KOH as shown below and match the following: \(\mathrm{Br}_{2}+\mathrm{KOH} \rightarrow \mathrm{KBr}+\mathrm{KBrO}_{\mathrm{a}}+\mathrm{H}_{2} \mathrm{O}\) $$ \begin{array}{ll} \text { Column-I (Compound) } & \text { Column-II (n-Facto r) } \\ \hline \text { (a) } \mathrm{KOH} & \text { p. } 1 \\ \text { (b) } \mathrm{KBr} & \text { q. } 5 \\ \text { (c) } \mathrm{KBrO}_{3} & \text { r. } 5 / 3 \\ \text { (d) } \mathrm{Br}_{2} & \text { s. } 5 / 6 \\ & \text { t. } 2 \\ \hline \end{array} $$

The value of \(\mathrm{n}\) (the number of electrons) in the half equation in which \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\)is oxidized to chromate ion in alkali medium is

On heating \(1.763 \mathrm{~g}\) of hydrated \(\mathrm{BaCl}_{2}\) to dryness, \(1.505 \mathrm{~g}\) of anhydrous salt remained. Number of moles of \(\mathrm{H}_{2} \mathrm{O}\) present in one mole of the hydrated \(\mathrm{BaCl}_{2}\) is ______

Equivalent weight of a metal is \(4.5\) and the molecular weight of the chloride is 80 . The valency of the metal is

Find the number of moles of \(\mathrm{KCl}\) in \(1000 \mathrm{~mL}\) of \(3 \mathrm{M}\) solution.

\(\mathrm{g}\) of an acid \(\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{O}_{4}\) required \(0.768 \mathrm{~g}\) of \(\mathrm{KOH}\) for complete neutralization. Determine the basicity of acid.

When the equation \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+\mathrm{H}^{+}+\mathrm{I}^{-} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{I}_{2}\) Is balanced, give the correct coefficient for I (aq)

How many of the following depends upon temperature? Concentration, Normality, molarity, formality molality, mol fraction, \% by mass, \%by strength

Number of atoms in \(560 \mathrm{~g}\) of \(\mathrm{Fe}\) (atomic mass \(56 \mathrm{~g}\) \(\mathrm{mol}^{-1}\) ) is \(\quad[\mathbf{2 0 0 2}]\) (a) is twice that of \(70 \mathrm{~g} \mathrm{~N}\) (b) is half that of \(20 \mathrm{~g} \mathrm{H}\) (c) both are correct (d) none is correct

What volume of hydrogen gas, at \(273 \mathrm{~K}\) and \(1 \mathrm{~atm}\) pressure will be consumed in obtaining \(21.6 \mathrm{~g}\) of elemental boron (atomic mass \(=10.8\) ) from the reduction of boron trichloride by hydrogen? [2003] (a) \(89.6 \mathrm{~L}\) (b) \(67.2 \mathrm{~L}\) (c) \(44.8 \mathrm{~L}\) (d) \(22.4 \mathrm{~L}\)

\(7.25 \mathrm{~mL}\) of a solution of barium hydroxide on titration with \(0.1\) molar solution of hydrochloric acid gave a titre value of \(35 \mathrm{~mL}\). The molarity of barium hydroxide solution was (a) \(0.07\) (b) \(0.14\) (c) \(0.28\) (d) \(0.35\)

To neutralize completely \(20 \mathrm{~mL}\) of \(0.1 \mathrm{M}\) aqueous solution of phosphorus acid, the volume of \(0.1 \mathrm{M}\) aqueous KOH solution required is (a) \(10 \mathrm{~mL}\) (b) \(40 \mathrm{~mL}\) (c) \(60 \mathrm{~mL}\) (d) \(80 \mathrm{~mL}\)

\(.6 .02 \times 10^{20}\) molecules of urea are present in \(100 \mathrm{~mL}\) of its solution. The concentration of urea solution is [2004] (a) \(0.02 \mathrm{M}\) (b) \(0.001 \mathrm{M}\) (c) \(0.01 \mathrm{M}\) (d) \(0.1 \mathrm{M}\)

If we consider that \(\frac{1}{6}\), in place of \(\frac{1}{12}\), mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of a substance will \([\mathbf{2 0 0 5}]\) (a) decrease twice (b) increase two fold (c) remain unchanged (d) be a function of the molecular mass of the substance

How many moles of magnesium phosphate, \(\mathrm{Mg}_{3}\) \(\left(\mathrm{PO}_{4}\right)_{2}\) will contain \(0.25\) mole of oxygen atoms? (a) \(0.02\) (b) \(3.125 \times 10^{-2}\) (c) \(1.25 \times 10^{-2}\) (d) \(2.5 \times 10^{-2}\)

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 (a) \(1.14 \mathrm{~mol} \mathrm{~kg}^{-1}\) (b) \(3.28 \mathrm{~mol} \mathrm{~kg}^{-1}\) (c) \(2.28 \mathrm{~mol} \mathrm{~kg}^{-1}\) (d) \(0.44 \mathrm{~mol} \mathrm{~kg}^{-1}\)

The reaction, \(2 \mathrm{Al}(\mathrm{s})+6 \mathrm{HCl}\) (aq) \(\longrightarrow 2 \mathrm{Al}^{3+}\) (aq) $$ \begin{gathered} +6 \mathrm{Cl}^{-}(\mathrm{aq})+3 \mathrm{H}_{2}(\mathrm{~g}) \\ \text { [2007] } \end{gathered} $$ (a) \(33.6 \mathrm{~L} \mathrm{H}_{2}(\mathrm{~g})\) is produced regardless of temperature and pressure for every mole of \(\mathrm{Al}\) that reacts (b) \(67.2 \mathrm{~L} \mathrm{H}_{2}(\mathrm{~g})\) at STP is produced for every mole of Al that reacts (c) \(11.2 \mathrm{~L} \mathrm{H}_{2}(\mathrm{~g})\) at STP is produced for every mole of \(\mathrm{HCl}\) (aq) consumed (d) \(6 \mathrm{~L} \mathrm{HCl}\) (aq) is consumed for every \(3 \mathrm{~L} \mathrm{H}_{2}(\mathrm{~g})\) produced

The density (in \(\mathrm{g} \mathrm{mL}^{-1}\) ) of a \(3.60 \mathrm{M}\) sulphuric acid solution, that is, \(29 \% \mathrm{H}_{2} \mathrm{SO}_{4}\) (molar mass \(=98 \mathrm{~g}\) \(\mathrm{mol}^{-1}\) ) by mass will be \([\mathbf{2 0 0 7}]\) (a) \(1.88\) (b) \(1.22\) (c) \(1.45\) (d) \(1.64\)

A \(5.2\) molal aqueous solution of methyl alcohol, \(\mathrm{CH}_{3} \mathrm{OH}\), is supplied. What is the mole fraction of methyl alcohol in the solution? (a) \(0.86\) (b) \(0.086\) (c) \(0.043\) (d) \(1.0\)

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 solutions is: [2012] (a) \(1.02 \mathrm{M}\) (b) \(0.50 \mathrm{M}\) (c) \(2.05 \mathrm{M}\) (d) \(1.78 \mathrm{M}\)

The molarity of a solution obtained by mixing 750 \(\mathrm{mL}\) of \(0.5(\mathrm{M}) \mathrm{HCl}\) with \(250 \mathrm{~mL}\) of \(2(\mathrm{M}) \mathrm{HCl}\) will be (a) \(1.75 \mathrm{M}\) (b) \(0.975 \mathrm{M}\) (c) \(0.875 \mathrm{M}\) (d) \(1.78 \mathrm{M}\)

The molecular formula of a commercial resin used for exchanging ions in water softening is \(\mathrm{C}_{8} \mathrm{H}_{7} \mathrm{SO}_{3} \mathrm{Na}\) (mol. wt. 206). What would be the maximum uptake of \(\mathrm{Ca}^{2+}\) ions by the resin when expressed in mole per gram resin? (a) \(\frac{1}{103}\) (b) \(\frac{1}{206}\) (c) \(\frac{2}{309}\) (d) \(\frac{1}{412}\)