Chapter 1

The amount of Zinc (atomic weight \(=65\) ) necessary to produce \(224 \mathrm{~mL}\) of \(\mathrm{H}_{2}\) by the reaction with an acid will be (a) \(0.65 \mathrm{~g}\) (b) \(7.6 \mathrm{~g}\) (c) \(6.5 \mathrm{~g}\) (d) \(8.5 \mathrm{~g}\)

Assuming fully decomposed, the volume of \(\mathrm{CO}_{2}\) released at STP on heating \(9.85 \mathrm{~g}\) of \(\mathrm{BaCO}_{3}\) (atomic mass, \(\mathrm{Ba}=137\) ) will be (a) \(1.12 \mathrm{~L}\) (b) \(4.84 \mathrm{~L}\) (c) \(2.12 \mathrm{~L}\) (d) \(2.06 \mathrm{~L}\)

Specific volume of cylindrical virus particle is \(6.02 \times\) \(10^{-2} \mathrm{cc} / \mathrm{g}\). Whose radius and length are \(7 \AA\) and \(10 \AA\) respectively. If \(\mathrm{N}_{\mathrm{A}}=6.02 \times 10^{23}\), find molecular weight of virus (a) \(15.4 \mathrm{~kg} / \mathrm{mol}\) (b) \(1.54 \times 10^{4} \mathrm{~kg} / \mathrm{mol}\) (c) \(4.68 \times 10^{4} \mathrm{~kg} / \mathrm{mol}\) (d) \(2.08 \times 10^{3} \mathrm{~kg} / \mathrm{mol}\)

\(500 \mathrm{~mL}\) 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 \(6.02 \times\) \(10^{24} \mathrm{CO}\) molecules is (a) \(10 \mathrm{~g}\) molecules (b) \(5 \mathrm{~g}\) molecules (c) 1 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 \(4 \mathrm{NH}_{3}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(1)\) 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 NO will be produced (c) all the ammonia will be consumed (d) all the oxygen will be consumed

Pressure in a mixture of \(4 \mathrm{~g}\) of \(\mathrm{O}_{2}\) and \(2 \mathrm{~g}\) of \(\mathrm{H}_{2}\) confined in a container of 1 litre capacity at \(0{ }^{\circ} \mathrm{C}\) is (a) \(25.2 \mathrm{~atm}\) (b) \(35.6 \mathrm{~atm}\) (c) \(15.4 \mathrm{~atm}\) (d) \(48.2 \mathrm{~atm}\)

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 \(\mathrm{HCl}\) ? (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 \([\mathrm{Fe}(\mathrm{CN})]^{3-}\) is 60 .

The strength of "20 volume" \(\mathrm{H}_{2} \mathrm{O}_{2}\) is equal to (a) \(3.58 \mathrm{~N}\) (b) \(3.035 \%\) (c) \(60.86 \mathrm{~g} / \mathrm{L}\) (d) \(1.79 \mathrm{M}\)

\(100 \mathrm{ml}\) 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.

Oleum is considered as a solution of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\), which is obtained by passing \(\mathrm{SO}_{3}\) in concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\). When \(100 \mathrm{~g}\) sample of oleum is diluted with desired weight of \(\mathrm{H}_{2} \mathrm{O}\), then the total mass of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) obtained after dilution is known as \% labeling in oleum. For example, an oleum labeled as '109\% \(\mathrm{H}_{2} \mathrm{SO}_{4}\), means the \(109 \mathrm{~g}\) total mass of pure \(\mathrm{H}_{2} \mathrm{SO}_{4}\) will be formed when \(100 \mathrm{~g}\) of oleum is diluted by \(9 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) which combines with all the free \(\mathrm{SO}_{3}\) present in oleum to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) as \(\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}\). What is the \(\%\) of free \(\mathrm{SO}_{3}\) is an oleum that is labeled as \(104.5 \% \mathrm{H}_{2} \mathrm{SO}_{4}^{\prime} ?\) (a) 30 (b) 10 (c) 20 (d) 40

Oleum is considered as a solution of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\), which is obtained by passing \(\mathrm{SO}_{3}\) in concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\). When \(100 \mathrm{~g}\) sample of oleum is diluted with desired weight of \(\mathrm{H}_{2} \mathrm{O}\), then the total mass of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) obtained after dilution is known as \% labeling in oleum. For example, an oleum labeled as '109\% \(\mathrm{H}_{2} \mathrm{SO}_{4}\), means the \(109 \mathrm{~g}\) total mass of pure \(\mathrm{H}_{2} \mathrm{SO}_{4}\) will be formed when \(100 \mathrm{~g}\) of oleum is diluted by \(9 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) which combines with all the free \(\mathrm{SO}_{3}\) present in oleum to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) as \(\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}\). \(.9 .0 \mathrm{~g}\) water is added into oleum sample labeled as \(" 112 \% " \mathrm{H}_{2} \mathrm{SO}_{4}\) then the volume of free \(\mathrm{SO}_{3}\) remaining in the solution atl atm pressure and \(0^{\circ} \mathrm{C}\) is (a) \(7.46 \mathrm{~L}\) (b) \(3.73 \mathrm{~L}\) (c) \(11.2 \mathrm{~L}\) (d) \(7.34 \mathrm{~L}\)

Oleum is considered as a solution of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\), which is obtained by passing \(\mathrm{SO}_{3}\) in concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\). When \(100 \mathrm{~g}\) sample of oleum is diluted with desired weight of \(\mathrm{H}_{2} \mathrm{O}\), then the total mass of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) obtained after dilution is known as \% labeling in oleum. For example, an oleum labeled as '109\% \(\mathrm{H}_{2} \mathrm{SO}_{4}\), means the \(109 \mathrm{~g}\) total mass of pure \(\mathrm{H}_{2} \mathrm{SO}_{4}\) will be formed when \(100 \mathrm{~g}\) of oleum is diluted by \(9 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) which combines with all the free \(\mathrm{SO}_{3}\) present in oleum to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) as \(\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}\). \(1 \mathrm{~g}\) of oleum sample is diluted with water. The solution required \(54 \mathrm{~mL}\) of \(0.4 \mathrm{~N} \mathrm{NaOH}\) for complete neutralization. The \(\%\) of free \(\mathrm{SO}_{3}\) in the sample is (a) 20 (b) 52 (c) 26 (d) none of these

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 ___ .

Consider the reaction, \(3 \mathrm{Br}_{2}+6 \mathrm{NaOH} \longrightarrow 5 \mathrm{NaBr}+\) \(\mathrm{NaBrO}_{3}+3 \mathrm{H}_{2} \mathrm{O} .\) If \(\mathrm{E}\) and \(\mathrm{A}\) represent equivalent weight and atomic weight of bromine, then \(5 \mathrm{E}=\mathrm{x} \mathrm{A}\). The value of \(x\) is ____ .

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

\(1 \mathrm{~g}\) 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 \(\mathrm{I}^{-}\)(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 \(56 \mathrm{~g}\) \(\left.\mathrm{mol}^{-1}\right)\) is (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 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) \(22.4 \mathrm{~L}\)

\(25 \mathrm{~mL}\) 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 [2004] (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 (a) \(0.02 \mathrm{M}\) (b) \(0.001 \mathrm{M}\) (c) \(0.01 \mathrm{M}\) (d) \(0.1 \mathrm{M}\)

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) \(0.44 \mathrm{~mol} \mathrm{~kg}^{-1}\)

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) \(\frac{1}{412}\)