201. One gram of hydrogen is found to combine with \(80 \mathrm{~g}\) of bromine. One gram of calcium (Valency \(=2\) ) combines with \(4 \mathrm{~g}\) of bromine. The equivalent weight of calcium is

1) 10

2) 20

3) 40

4) 80

202. A mixture of \(\mathrm{CH}_{4}, \mathrm{~N}_{2}\) and \(\mathrm{O}_{2}\) is enclosed in a vessel of one litre capacity at \(0^{\circ} \mathrm{C}\). The ratio of particle pressures of gases is \(1: 4: 2\). Total pressure of the gaseous mixture is \(2660 \mathrm{~mm}\). the number of molecules of oxygen present in the vessel is

1) \(\frac{6.02 \times 10^{23}}{22.4}\)

2) \(6.02 \times 10^{23}\)

3) \(22.4 \times 10^{22}\)

4) 1000

203. A \(400 \mathrm{mg}\) iron capsule contains \(100 \mathrm{mg}\) of ferrous fumarate, \((\mathrm{CHCOO})_{2} \mathrm{Fe}\). the percentage of iron present in it is approximately

1) \(33 \%\)

2) \(25 \%\)

3) \(14 \%\)

4) \(8 \%\)

204. A certain amount of a metal whose equivalent mass is 28 displaces \(0.7 \mathrm{~L}\) of \(\mathrm{H}_{2}\) at STP from an acid. Hence, mass of the element is

1) \(1.75 \mathrm{~g}\)

2) \(0.875 \mathrm{~g}\)

3) \(3.50 \mathrm{~g}\)

4) \(7.00 \mathrm{~g}\)

\(205.100 \mathrm{~mL}\) of \(20.8 \% \mathrm{BaCl}_{2}\) solution and \(50 \mathrm{~mL}\) of \(9.8 \% \mathrm{H}_{2} \mathrm{SO}_{4}\)

Solution will form \(\mathrm{BaSO}_{4}\)

\((B a=137, C l=35.5, S=32, H=1,0=16\)

\(\mathrm{BaCl}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{Ba}_{2} \mathrm{SO}_{4}+2 \mathrm{HCl}\)

1) \(23.3 \mathrm{~g}\)

2) \(11.65 \mathrm{~g}\)

3) \(30.6 \mathrm{~g}\)

4) None of these

206. A sample of a mixture of \(\mathrm{CaCl}_{2}\) and \(\mathrm{NaCl}\) weighing \(4.22 \mathrm{~g}\) was treated to precipitate all the \(\mathrm{Ca}\) as \(\mathrm{CaCO}_{3}\). This \(\mathrm{CaCO}_{3}\) is then heated and quantitatively converted into \(0.959 \mathrm{~g}\) of \(\mathrm{CaO}\). Calculate the percentage of \(\mathrm{CaCl}_{2}\) in the mixture.

(Atomic mass of \(C a=40, O=16, C=12\) and \(\mathrm{Cl}=35.5)\)

1) \(31.5 \%\)

2) \(21.5 \%\)

3) \(45.04 \%\)

4) \(68.48 \%\)

207. A metal nitride, \(M_{3} N_{2}\) contains \(28 \%\) of nitrogen. The atomic mass of metal, \(M\) is

1) 24

2) 54

3) 9

4) 87.62 208. If \(20 \mathrm{~g}\) of \(\mathrm{CaCO}_{3}\) is treated with \(100 \mathrm{~mL}\) of \(20 \%\) \(\mathrm{HCl}\) solution, the amount of \(\mathrm{CO}_{2}\) produced is

1) \(22.4 \mathrm{~L}\)

2) \(8.80 \mathrm{~g}\)

3) \(4.40 \mathrm{~g}\)

4) \(2.24 \mathrm{~L}\)

209.1.520 \(\mathrm{g}\) of the hydroxide of a metal on ignition gave \(0.995 \mathrm{~g}\) of oxide. The equivalent weight of metal is

1) 1.520

2) 0.995

3) 19.00

4) 9.00

210. If isotopic distribution of C-12 and C-14 is \(98 \%\) and \(2 \%\) respectively then the number of C-14 atoms in \(12 \mathrm{~g}\) of carbon is

1) \(1.032 \times 10^{22}\)

2) \(3.01 \times 10^{22}\)

3) \(5.88 \times 10^{23}\)

4) \(6.023 \times 10^{23}\)

211. The law of definite proportions is not applicable to nitrogen oxide because 1) Nitrogen atomic 2) Nitrogen molecular weight is not weight is variable constant

3) Nitrogen equivalent 4) Oxygen atomic weight is variable weight is variable

212.0.75 moles of a solid \(A_{4}\) and 2 moles of \(O_{2}(g)\)

are heated in a sealed vessel, completely using up the reactants and produces only one compound. It is found that when the temperature is used to initial temperature, the contents of the vessel exhibit a pressure equal to \(\frac{1}{2}\) of the original pressure. The formula of the product will be

1) \(\mathrm{A}_{2} \mathrm{O}_{3}\)

2) \(A_{3} O_{8}\)

3) \(\mathrm{A}_{3} \mathrm{O}_{4}\)

4) \(\mathrm{AO}_{2}\)

213. \(x\) g of \(\mathrm{Ag}\) was dissolved in \(\mathrm{HNO}_{3}\) and the solution was treated with excess of \(\mathrm{NaCl}\) when \(2.87 \mathrm{~g}\) of \(\mathrm{AgCl}\) was precipitated. The value of \(x\) is

1) \(1.08 \mathrm{~g}\)

2) \(2.16 \mathrm{~g}\)

3) \(2.70 \mathrm{~g}\)

4) \(1.62 \mathrm{~g}\)

214. What quantity of ammonium sulphate is necessary for the production of \(\mathrm{NH}_{3}\) gas sufficient to neutralize a solution containing \(292 \mathrm{~g}\) of \(\mathrm{HCl}\) ?

\(\left[\mathrm{HCl}=36.5,\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}=132, \mathrm{NH}_{3}=17\right]\)

1) \(272 \mathrm{~g}\)

2) \(403 \mathrm{~g}\)

3) \(528 \mathrm{~g}\)

4) \(1056 \mathrm{~g}\)

215. What weight of silver chloride will be precipitated when a solution containing \(4.77 \mathrm{~g}\) of \(\mathrm{NaCl}\) is added to a solution of \(5.77 \mathrm{~g}\) of \(\mathrm{AgNO}_{3} ?(\mathrm{Na}=23, \mathrm{Cl}=35.5, \mathrm{Ag}=108, \mathrm{~N}=\) and \(O=16\) )

1) \(4.37 \mathrm{~g}\)

2) \(4.87 \mathrm{~g}\)

3) \(5.97 \mathrm{~g}\)

4) \(3.87 \mathrm{~g}\)

216. The number of moles of oxygen in one litre of air containing \(21 \%\) oxygen by volume, in standard conditions, is

1) \(0.186 \mathrm{~mol}\)

2) \(0.21 \mathrm{~mol}\)

3) \(2.10 \mathrm{~mol}\)

4) \(0.0093 \mathrm{~mol}\)

217. There are two isotopes of an element with atomic massz. Heavier one has atomic mass \(z+2\) and lighter one has \(z-1\), the abundance of lighter one is

1) \(66.6 \%\)

2) \(69.7 \%\)

3) \(6.67 \%\)

4) \(33.3 \%\)

218. An ore contains \(1.34 \%\) of the mineral argentite, \(\mathrm{Ag}_{2} \mathrm{~S}\), by mass. How many gram of this ore would have to be processed in order to obtain \(1.00 \mathrm{~g}\) of pure solid silver, \(A g\) ?

1) \(74.6 \mathrm{~g}\)

2) \(85.7 \mathrm{~g}\)

3) \(107.9 \mathrm{~g}\)

4) \(134.0 \mathrm{~g}\)

\section{Multiple Correct Answers Type}

219. Avogadro's number is the number of molecules present in

1) 32 g of oxygen

2) \(1 \mathrm{~g}\) molecule of a substance

3) 22.4 L if a gas at NTP 4) None of the above

220 . Which of the following is isomorphous with magnesium sulphate \(\left(\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\right)\) ?

1)Green vitriol

2)Potassium perchlorate

3)Zinc sulphate hepta 4)Blue vitriol hydrate

221. Which of the following has three significant figures?

1) 3.70

2) \(6.23 \times 10^{25}\)

3) 1.03

4) 0.052

222. Which of the following relationships are wrong?

1) \(1 \mathrm{~atm}=760 \mathrm{~cm} \mathrm{Hg}\)

\(1 \mathrm{eV}=1.6021\)

\(\times 10^{-19} \mathrm{cal}\)

3) \(1 u=931.43 \mathrm{eV}\)

4) 1 dyne \(=10^{-5} \mathrm{~N}\)

223.2.0 \(\mathrm{g}\) of a triatomic gaseous element was found to occupy a volume of \(448 \mathrm{~mL}\) at \(76 \mathrm{~cm}\) of \(\mathrm{Hg}\) and \(273 \mathrm{~K}\). the mass of its atom is

1) \(38.5 \mathrm{~g}\)

2) \(33.3 u\)

3) \(5.53 \times 10^{-23} \mathrm{~g}\)

4) \(38.5 \mathrm{u}\)

\section{Assertion - Reasoning Type}

This section contain(s) 11 question(s) numbered 224 to 234. Each question contains STATEMENT 1(Assertion) and STATEMENT 2(Reason). Each question has the 4 choices (1), (2), (3) and (4) out of which ONLY ONE is correct.

1) Statement 1 is True, Statement 2 is True;

Statement 2 is correct explanation for Statement 1 2) Statement 1 is True, Statement 2 is True; Statement 2 is not correct explanation for Statement 1

3) Statement 1 is True, Statement 2 is False

4) Statement 1 is False, Statement 2 is True 224

Statement 1: Equal moles of different substances contain same number of constituent particles.

Statement 2: Equal weights of different substances contain the same number of constituent particles. The correct answer is

225

Statement 1: Equivalent weight of ozone in the change \(\mathrm{O}_{3} \rightarrow 0_{2}\) is 8 .

Statement 2: 1 mole \(O_{3}\) of on decomposition gives \(\frac{3}{2}\) moles of \(\mathrm{O}_{2}\).

226

Statement 1: Equivalent of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) has 1 equivalent of \(\mathrm{K}\) and \(\mathrm{Cr}\) and \(\mathrm{O}\) each.

Statement 2: A species contains same number of equivalents of its components.

227

Statement 1: The molality of the solution does not change with change in temperature.

Statement 2: The molality of the solution is expressed in units of moles per \(1000 \mathrm{~g}\) of solvent.

228

Statement 1: Normally and molarity can be calculated from each other.

Statement 2: Normally is equal to the product of molarity and \(n\).

229

Statement 1: A solution which contains one gram equivalent of solute per litre of solutions is known as molar solution

Statement 2: Normality=normality \(\times \frac{\text { mol.wt.of solute }}{\text { eq.wt.of solute }}\)

230

Statement 1: \(\quad 10,000\) molecules of \(\mathrm{CO}_{2}\) have the same volume at STP as 10,000 molecules of \(C O\) at STP. Statement 2: Both \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\) are formed by combustion of carbon in presence of oxygen.

231

Statement 1: Molality and mole fraction are not affected by temperature.

Statement 2: \(\quad\) Molality \((m)=\frac{W}{G M M} \times \frac{1}{b}\) (where, \(b=\) mass of solven). 232

Statement 1: The percentage of nitrogen in urea is \(46.6 \%\)

Statement 2: Urea is an ionic compound. 233

Statement 1: Strength of a solution is \(10,000 x \mathrm{~g}\) in one litre.

Statement 2: \(10 x\) of solute is dissolved in 1 mL solution.

234

Statement 1: Weight of 1 molecule of \(\mathrm{O}_{2}=32 \mathrm{u}\)

Statement 2: 1 g molecule \(=6.023 \times 10^{23}\) molecules.

\section{Matrix-Match Type}

This section contain(s) 1 questions. Each question contains Statements given in 2 columns which have to be matched. Statements in columns I have to be matched with Statements in columns II. 235 Match the following List I and List II.

Column-I

Column- II

(A) \(10 \mathrm{~g}\) \(\mathrm{CaCO}_{3}\)

(1) \(0.224 \mathrm{~L} \mathrm{CO}_{2}\)

(B) \(1.06 \mathrm{~g}\)

(2) \(4.48 \mathrm{~L} \mathrm{CO}_{2}\) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) Excess \(\mathrm{HC}\)

\(\begin{array}{ll}\text { (C) } 2.4 \mathrm{~g} \mathrm{C} & \text { (3) } 0.448 \mathrm{~L} \mathrm{CO}_{2}\end{array}\) \(\operatorname{Excess}_{2} \rightarrow\)

\(\begin{array}{ll}\text { (D) } 0.56 \mathrm{~g} \mathrm{CO} & \text { (4) } 2.24 \mathrm{~L} \mathrm{CO}_{2}\end{array}\) \(\operatorname{Excess~}_{2} \rightarrow\)

(5) \(22.4 \mathrm{~L} \mathrm{CO}_{2}\)

Codes :

\(\begin{array}{lllll} & \text { A } & \text { B } & \text { C } & \text { D } \\ (1) & 4 & 1 & 2 & 3 \\ (2) & 5 & 1 & 2 & 3 \\ (3) & 4 & 1 & 3 & 2 \\ (4) & 1 & 4 & 2 & 3\end{array}\)

Linked Comprehension Type

This section contain(s) 2 paragraphs. Based upon each paragraph, multiple choice questions have to be answered. Each question has at least 4 choices (a), (b), (c) and (d) out of which ONLY ONE is correct.

\section{Paragraph for Question Nos. 236 - 238}

Mole is a unit which represents \(6.02 \times 10^{23}\) particles (atoms, molecules or ions etc) irrespective of the nature. The number \(6.023 \times 10^{23}\) is called avogadros number and is represented by \(N_{0}\). The calculation of the number is based on the Faradys law of electrolysis. A mole also represents gram molecular mass (GMM) of the substance.

236. The number of moles \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) in \(13.5 \mathrm{~g}\) is

1) 0.25

2) 1.5

3) 0.4

4) 0.1

237.How many atoms are present in a mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) ?

1) \(7 \times 6.02 \times 10^{23}\)

2) \(1.5 \times 6.02 \times 10^{23}\)

3) \(6.02 \times 10^{23}\)

4) \(2 \times 6.02 \times 10^{23}\)

238. The number o potassium atoms in 2 moles of potassium ferricyanide is

1) \(36.13 \times 10^{23}\)

2) \(6.02 \times 10^{23}\)

3) \(24.08 \times 10^{23}\)

4) \(2 \times 10^{23}\)

Paragraph for Question Nos. 239 - 241

The atomic mass of an atom (element) is not its actual mass. It is relative mass as compared with an atom of carbon taken as 12 . It is expressed in amu (u). the actual mass of an atom means its mass in grams which is obtained by dividing the atomic mass of the element by Avogadro's number \(\left(6.02 \times 10^{23}\right)\) because one gram atom contains Avogadro's number of atoms.

239.Which of the following has maximum mass?

1) 0.1 moles of

2) 1120 cc of carbon ammonia dioxide

3) \(0.1 \mathrm{~g}\) atom of carbon 4) \(\begin{aligned} & 6.02 \times 10^{22} \text { molecules }\end{aligned}\)

240.The mass of one atom of hydrogen is approximately

1) \(1 \mathrm{~g}\)

2) \(3.2 \times 10^{-24} \mathrm{~g}\)

3) \(1.6 \times 10^{-24} \mathrm{~g}\)

4) \(0.5 \mathrm{~g}\)

241.5.6 L of a gas at NTP are found to have a mass of \(11 \mathrm{~g}\). the molecular mass of the gas is

1) 36

2) 48

3) 40

4) 44