101.The stoichiometry of the following reaction is

\(\mathrm{K}_{2} \mathrm{~S}_{2} \mathrm{O}_{8}(a q)+2 \mathrm{KI}(a q) \rightarrow 2 \mathrm{~K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{I}_{2}(a q)\)

[J\&K CET 2008]

1) \(2: 2\)

2) \(1: 1\)

3) \(1: 2\)

4) \(2: 1\)

102. Air contains \(20 \% \mathrm{O}_{2}\) by volume. How much volume of air will be required for \(100 \mathrm{cc}\) of acetylene? [DCE 2007]

1) \(500 \mathrm{cc}\)

2) \(1064 \mathrm{cc}\)

3) \(212.8 \mathrm{cc}\)

4) \(1250 \mathrm{cc}\)

103. For the reaction, \(\mathrm{Fe}_{2} \mathrm{O}_{3}+3 \mathrm{CO} \rightarrow 2 \mathrm{Fe}+3 \mathrm{CO}_{2}\) the volume of carbon monoxide required to reduce one mole of ferric oxide is [KCET 2008]

1) \(22.4 \mathrm{dm}^{3}\)

2) \(44.8 \mathrm{dm}^{3}\)

3) \(67.2 \mathrm{dm}^{3}\)

4) \(11.2 \mathrm{dm}^{3}\)

104.Consider a titration of potassium dichromate solution with acidified Mohr's salt solution using diphenylamine as indicator. The number of moles of Mohr's salt required per mole of dichromate is [IIT JEE 2007]

1) 3

2) 4

3) 5

4) 6

105. Mixture \(X=0.02\) mole of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{SO}_{4}\right] \mathrm{Br}\) and 0.02 mole of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Br}^{\mathrm{SO}} \mathrm{SO}_{4}\right.\) was prepared in \(2 \mathrm{~L}\) of solution.


1 Lof mixture \(X+\) excess \(\mathrm{BaCl}_{2} \rightarrow Z\)

Number of moles of \(Y\) and \(Z\) are [IIT JEE

2003]

1) \(0.01,0.01\)

2) \(0.02,0.01\)

3) \(0.01,0.02\)

4) \(0.02,0.02\)

106. When \(10 \mathrm{~g}\) of methane is completely burnt in oxygen, the heat evolved is \(560 \mathrm{~kJ}\). What is the heat of combustion (in \(\mathrm{kJ} \mathrm{mol}^{-1}\) ) of methane?

[EAMCET 2003]

1) -1120

2) -968

3) -896

4) -560

107. The mass of potassium dichromate crystals required to oxidise \(750 \mathrm{~cm}^{3}\) of \(0.6 \mathrm{M} \mathrm{Mohr's}\) salt solution is (Given, molar mass : Potassium dichromate \(=294\), Mohr's salt \(=392)\) [AIEEE 2011]

1) \(0.49 \mathrm{~g}\)

2) \(0.45 \mathrm{~g}\)

3) \(22.05 \mathrm{~g}\)

4) \(2.2 \mathrm{~g}\)

108. 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 \(\mathrm{KOH}\) required to completely neutralise the gas is [Jamia Millia Islamia 2008]

1) \(56 \mathrm{~g}\)

2) \(28 \mathrm{~g}\)

3) \(42 \mathrm{~g}\)

4) \(20 \mathrm{~g}\)

109. Sodium bicarbonate on heating decomposes to form sodium carbonate, \(\mathrm{CO}_{2}\) and water. If 0.2 moles of sodium bicarbonate is completely decomposed, how many moles of sodium carbonate is formed? [J\&K CET 2006]

1) 0.1

2) 0.2

3) 0.05

4) 0.025

110. The mass of \(\mathrm{BaCO}_{3}\) produced when excess \(\mathrm{CO}_{2}\) is bubbled through a solution of 0.205 mole \(\mathrm{Ba}\) \((\mathrm{OH})_{2}\) is, [UP SEE 2004]

1) \(81 \mathrm{~g}\)

3) \(20.25 \mathrm{~g}\)

2) \(40.5 \mathrm{~g}\)

4) \(162 \mathrm{~g}\)

111.100 g of \(\mathrm{CaCO}_{3}\) is treated with \(1 \mathrm{~L}\) of \(1 \mathrm{~N} \mathrm{HCI}\). What would be the weight of \(\mathrm{CO}_{2}\) liberated after the completion of the reaction?

[Kerala CEE 2005]

1) \(55 \mathrm{~g}\)

2) \(11 \mathrm{~g}\)

3) \(22 \mathrm{~g}\)

4) \(33 \mathrm{~g}\)

5) \(44 \mathrm{~g}\)

112. On combustion of \(4 \mathrm{~g}\) of the methane, \(10.46 \mathrm{~kJ}\) of heat is liberated. Heat of combustion of methane is [MP PET 2003]

1) \(83.68 \mathrm{~kJ}\)

2) \(10.46 \mathrm{~kJ}\)

3) \(41.84 \mathrm{~kJ}\)

4) \(20.93 \mathrm{~kJ}\)

113. What is the weight of oxygen that is required for the complete combustion of \(2.8 \mathrm{~kg}\) of ethylene? [BCECE 2006]

1) \(9.6 \mathrm{~kg}\)

2) \(96.0 \mathrm{~kg}\)

3) \(6.4 \mathrm{~kg}\)

4) \(2.8 \mathrm{~kg}\)

114. When \(10 \mathrm{~g}\) of \(90 \%\) pure lime stone is heated completely, the volume (in litres) of \(\mathrm{CO}_{2}\) is liberated at STP is [RPET 2007]

1) 22.4

2) 2.24

3) 20.16

4) 2.016

115. \(\mathrm{KMnO}_{4}\) reacts with oxalic acid according to the equation

\(2 \mathrm{MnO}_{4}^{-}+5 \mathrm{C}_{2} \mathrm{O}_{4}^{2-}+16 \mathrm{H}^{+} \rightarrow 2 \mathrm{Mn}^{2^{+}}+10 \mathrm{CO}_{2}-\) Here, \(20 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{KMnO}_{4}\) is equivalent to

\section{[J\&K CET 2003]}

 3) \(50 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{H}_{2} \mathrm{C}_{2}\) ) \(20 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{H}_{2} \mathrm{C}_{2}\)

116. The enthalpy of combustion of methane at \(25^{\circ} \mathrm{C}\) is \(890 \mathrm{~kJ}\). The heat liberated when \(3.2 \mathrm{~g}\) of methane is burnt in air is [AMU 2006]

1) \(445 \mathrm{~kJ}\)

2) \(278 \mathrm{~kJ}\)

3)-890 kJ

4) \(178 \mathrm{~kJ}\)

117. What amount of bromine will be required to convert \(2 \mathrm{~g}\) of phenol into 2, 4, 6-tribromo phenol? [UP SEE 2007]

1) \(20.44 \mathrm{~g}\)

2) \(6.00 \mathrm{~g}\)

3) \(4.00 \mathrm{~g}\)

4) \(10.22 \mathrm{~g}\)

118. Amount of oxalic acid present in a solution can be determined by its titration with \(\mathrm{KMnO}_{4}\) solution in the presence of \(\mathrm{H}_{2} \mathrm{SO}_{4}\). The titration given unsatisfactory result when carried out in the presence of \(\mathrm{HCl}\) because \(\mathrm{HCl}\) [AIEEE 2008] 1) Gets oxidised by Furnishes \(H^{+}\)ions in oxalic acid to chlorine reduces

2) addition to those from oxalic acid

4) Oxidises oxalic acid

3) permanganate to to carbon dioxide \(M n^{2^{+}}\) and water

119. In the reaction, \(2 A l(s)+6 H C l(a q) \rightarrow 2 A l^{3+}(a q)+6 C l^{-}(a q)+\) [AIEEE 2007]

\(6 \mathrm{~L} \mathrm{HCl}(a q)\) is 1) consumed for every \(3 \mathrm{~L} \mathrm{H}_{2}(g)\) produced

33. \(6 \mathrm{LH}_{2}(g)\) is produced regardless

2) of temperature and pressure for every mole \(\mathrm{Al}\) that reacts

67. \(2 \mathrm{~L} \mathrm{H}_{2}(g)\) at STP 11. \(2 \mathrm{LH}_{2}(g)\) at STP

3 ) is produced for every mole \(\mathrm{Al}\) that

4) is produced for every reacts mole \(\mathrm{HCl}(a q)\) consumed

120.2.76 g of silver carbonate on being strongly heated yield a residue weighing [Jamia Millia Islamia 2004]

1) \(2.16 \mathrm{~g}\)

2) \(2.48 \mathrm{~g}\) 

3) \(2.64 \mathrm{~g}\)

4) \(2.32 \mathrm{~g}\)

121. \(\mathrm{MnO}_{4}^{-}\)ions are reduced in acidic condition to \(M n^{2+}\) ions whereas they are reduced in neutral condition to \(\mathrm{MnO}_{2}\). The oxidation of \(25 \mathrm{~mL}\) of a solution \(X\) containing \(F e^{2+}\) ions required in acidic condition \(20 \mathrm{~mL}\) of a solution \(Y\) containing \(\mathrm{MnO}_{4}^{-}\)ions. What volume of solution \(Y\) would be required to oxidise \(25 \mathrm{~mL}\) of a solution \(X\) containing \(\mathrm{Fe}^{2^{+}}\)ions in neutral condition? [Kerala CEE 2008]

1) \(11.4 \mathrm{~mL}\)

2) \(12.0 \mathrm{~mL}\)

3) \(33.3 \mathrm{~mL}\)

4) \(35.0 \mathrm{~mL}\)

5) \(25.0 \mathrm{~mL}\)

122. Acidified \(\mathrm{KMnO}_{4}\) oxidises oxalic acid to \(\mathrm{CO}_{2}\).

What is the volume (in litres) of \(10^{-4} \mathrm{M} \mathrm{KMnO}_{4}\) required to completely oxidise \(0.5 \mathrm{~L}\) of \(10^{-2} \mathrm{M}\) oxalic acid in acid medium? [DCE 2008]

1) 125

2) 1250

3) 200

4) 20

123.1 mole of methyl amine on reaction with nitrous acid gives at NTP [WB JEE 2008]

1) \(1.0 \mathrm{~L}\) of nitrogen

2) \(22.4 \mathrm{~L}\) of nitrogen

3) \(11.2 \mathrm{~L}\) of nitrogen

4) \(5.6 \mathrm{~L}\) of nitrogen

124. 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? [DCE 2003]

1) \(89.6 \mathrm{~L}\)

2) \(67.2 \mathrm{~L}\)

3) \(44.8 \mathrm{~L}\)

4) \(22.4 \mathrm{~L}\)

125. A mixture of \(\mathrm{CaCl}_{2}\) and \(\mathrm{NaCl}\) weighing \(4.44 \mathrm{~g}\) is treated with sodium carbonate solution to precipitate all the \(\mathrm{Ca}^{2^{+}}\)ions as calcium carbonate. The calcium carbonate so obtained is heated strongly to get \(0.56 \mathrm{~g}\) of \(\mathrm{CaO}\). The percentage of \(\mathrm{NaCl}\) in the mixture (atomic mass of \(C a=40\) ) is [KCET 2010]

1) 75

2) 30.6

3) 25

4) 69.4

126. In which of the following numbers all zeros are significant?

1) 0.500

2) 30.000

3) 0.00030

4) 0.0050

127. The units \(\mathrm{J} \mathrm{Pa} \mathrm{P}^{-1}\) is equivalent to

1) \(m^{3}\)

2) \(\mathrm{cm}^{3}\)

3) \(d m^{3}\)

4) None of these

128. How many significant figures are there in (respectively)

(1) \(73.000 \mathrm{~g}\) (2) \(0.0503 \mathrm{~g}\) and (3) \(2.001 \mathrm{~s}\) ?

1) \(3,3,4\)

2) \(3,4,5\)

3) 2,5,4

4) 5,3,4

129. The answer of the calculation \(\frac{2.568 \times 5.8}{4.168}\) in significant figures will be

1) 3.579

2) 3.570

3) 3.57

4) 3.6

130.0.003924 have ....... significant figures.

1) 6

2) 4

3) 3

4) 7

131.The number of significant figures in Avogadro's number is

1) Four

2) Two

3) Three

4) Can be any of these

132. In multiplication and division, the significant figures of answer must be same as that in the quantity with ............ Number of significant figures.

1) Maximum

2) 3

3) 2

4) Minimum

133. Which of the following is not a mixture?

1) Gasoline

2) Distilled alcohol

3) LPG

4)lodized table salt

134.An example of homogeneous mixture is

1) Mixture of soil and 2) Mixture of salt and water sand grains

3) Sugar solution

4) None of the above

135. The smallest matter particle that can take part in chemical reaction is

1)Atom

2) Molecule

3) Both (a) and (b)

4) None of these

136. Matter is anything which occupies ...A... and has ... \(B \ldots\)

Here \(A\) and \(B\) are

1) Density and mass

2) Volume and mass

3) Space and mass

4) None of these

137. The solid like conducting state of gases with free electrons is called

1) Sol state

2) Gel state

3)Plasma state

4)All of these

138. The number of atoms present in a \(0.635 \mathrm{~g}\) of \(\mathrm{Cu}\) piece will be

1) \(6.023 \times 10^{-23}\)

2) \(6.023 \times 10^{23}\)

3) \(6.023 \times 10^{22}\)

4) \(6.023 \times 10^{21}\)

139. Number of molecules in \(100 \mathrm{~mL}\) of each of \(O_{2}\),

\(\mathrm{NH}_{3}\) and \(\mathrm{CO}_{2}\) at STP are in the order

1) \(\mathrm{CO}_{2}<\mathrm{O}_{2}<\mathrm{NH}_{3}\)

2) \(\mathrm{NH}_{3}<\mathrm{O}_{2}<\mathrm{CO}_{2}\)

3) \(\mathrm{NH}_{3}=\mathrm{CO}_{2}<\mathrm{O}_{2}\)

4) All have same number of molecules

140 . The sample with largest number of atoms is

1) \(1 \mathrm{~g}\) of \(O_{2}(g)\)

2) \(1 \mathrm{~g}\) of \(\mathrm{Ni}(s)\)

3) \(1 \mathrm{~g}\) of \(\mathrm{B}(s)\)

4) \(1 \mathrm{~g}\) of \(N_{2}(g)\)

141.A signature written with carbon pencil weighs

\(1 \mathrm{mg}\). what is the number of carbon atoms present in the signature? 

1) \(6.02 \times 10^{20}\)

2) \(0.502 \times 10^{20}\)

3) \(5.02 \times 10^{23}\)

4) \(5.02 \times 10^{20}\)

142.19.7 \(\mathrm{kg}\) of gold was recovered from a smuggler. How many atoms of gold were recovered \((\mathrm{Au}=\) 197)?

1) 100

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

3) \(6.02 \times 10^{24}\)

4) \(6.02 \times 10^{25}\)

143. How many moles of \(\operatorname{MgIn}_{2} S_{4}\) can be made from \(1 \mathrm{~g}\) each of \(M g\), in and S? (Atomic mass : \(\mathrm{Mg}=\) 24, , In \(=114.8, S=32\) )

1) \(6.47 \times 10^{-4}\)

2) \(3.0 \times 10^{-1}\)

3) \(9.17 \times 10^{-2}\)

4) \(8.7 \times 10^{-3}\)

144. How many gram of KCL would have to be dissolved in \(60 \mathrm{~g}_{2} \mathrm{O}\) to give \(40 \%\) by weight of solution?

1) \(40 \mathrm{~g}\)

2) \(20 \mathrm{~g}\)

3) \(15 \mathrm{~g}\)

4) \(10 \mathrm{~g}\)

145. The molecular weight of air will be (the components of air given as \(N_{2}-78 \%, O_{2}-21 \%, \mathrm{Ar}-09 \%\) and \(\left.\mathrm{CO}_{2}-0.1 \%\right)\)

1) 18.64

2) 24.968

3) 28.964

4) 29.864

146. If an iodized salt contains \(1 \% \mathrm{KI}\) and a person takes \(2 \mathrm{~g}\) of the salt every day, the iodide ions going into his body every day would be approximately

1) \(7.2 \times 10^{21}\)

2) \(7.2 \times 10^{19}\)

3) \(3.6 \times 10^{21}\)

4) \(9.5 \times 10^{19}\)

147. If the density of water is \(1 \mathrm{~g} \mathrm{~cm}^{-3}\) then the volume occupied by one molecule of water is approximately

1) \(18 \mathrm{~cm}^{3}\)

2) \(22400 \mathrm{~cm}^{3}\)

3) \(6.02 \times 10^{-23} \mathrm{~cm}^{3}\)

4) \(3.0 \times 10^{-23} \mathrm{~cm}^{3}\)

148. The mass of nitrogen per gram hydrogen in the compound hydrazine is exactly one and half times the mass of nitrogen in the compound ammonia. The fact illustrates the

1) Law of conservation 2) Multiple valency of of mass nitrogen

3) Law of multiple

4) Law of definite proportions proportions

149. The molarity of 20.0 mass \(\% \mathrm{H}_{2} \mathrm{SO}_{4}\) solution of density \(11.14 \mathrm{~g} \mathrm{~cm}^{-3}\) is

1) \(2.56 \mathrm{~mol} \mathrm{dm}\)

2) \(1.56 \mathrm{~mol} d m^{-3}\)

3) \(1.26 \mathrm{~mol} \mathrm{dm}^{-3}\)

4) \(2.32 \operatorname{mol} d m^{-3}\)

150. If \(6.3 \mathrm{~g}\) of \(\mathrm{NaHCO}_{3}\) are added to \(15.0 \mathrm{~g}\) \(\mathrm{CH}_{3} \mathrm{COOH}\) solution, the residue is found to weight \(18.0 \mathrm{~g}\). what is the mass of \(\mathrm{CO}_{2}\) released in the reaction?

1) \(4.5 \mathrm{~g}\)

2) \(3.3 \mathrm{~g}\)

3) \(2.6 \mathrm{~g}\)

4) \(2.8 \mathrm{~g}\)

151.A sample of copper sulphate pentahydrate contains \(8.64 \mathrm{~g}\) of oxygen. How many gram of \(\mathrm{Cu}\) is present in this sample?

(Atomic mass of \(\mathrm{Cu}=63.6, \mathrm{~S}=32.06,0=16\) )

1) \(0.952 \mathrm{~g}\)

2) \(3.816 \mathrm{~g}\)

3) \(3.782 \mathrm{~g}\)

4) \(8.64 \mathrm{~g}\)

152.If \(\mathrm{H}_{2} \mathrm{SO}_{4}\) ionises as

\(\mathrm{H}_{2} \mathrm{SO}_{4}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{SO}_{4}^{2}\), then total number of ions produced by \(0.1 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) will be

1) \(9.03 \times 10^{21}\)

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

3) \(6.02 \times 10^{22}\)

4) \(1.8 \times 10^{23}\)

153. A sample of \(A I F_{3}\) contains \(3.0 \times 10^{24} \mathrm{~F}\) ions.

The number of formula units of this sample are

1) \(9.0 \times 10^{24}\)

2) \(3.0 \times 10^{24}\)

3) \(0.75 \times 10^{24}\)

4) \(1.0 \times 10^{24}\)

154. One part of an element \(A\) combines with two parts of another element \(B .6\) parts of element \(C\) combines with 4 parts of \(B\). If \(A\) and \(C\) combine together, the ratio of their weights, will be governed by

1) Law of definite

2) Law of multiple proportions proportions

3) Law of reciprocal

4) Law of conservation proportions of mass

155. Calculate the number of moles left after removing \(10^{21}\) molecules from \(200 \mathrm{mg}\) of \(\mathrm{O}_{2}\).

1) 0.00454

2) 0.00166

3) \(2.88 \times 10^{-3}\)

4) None of these

156. A sample of ammonium phosphate \(\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}\) contains 6.36 moles of hydrogen atoms. The number of moles of oxygen atom in the sample is

(atomic mass of \(\mathrm{N}=14.04, \mathrm{H}=1, \mathrm{P}=31, \mathrm{O}=\) 16)

1) 0.265

2) 0.795

3) 2.12

4) 4.14

157. The mass of \(112 \mathrm{~cm}^{3}\) of \(\mathrm{CH}_{4}\) gas a STP is

1) \(0.16 \mathrm{~g}\)

2) \(0.8 \mathrm{~g}\)

3) \(0.08 \mathrm{~g}\)

4) \(1.6 \mathrm{~g}\)

158. The number of sodium atoms in 2 moles of sodium ferrocyanide is

1) \(12 \times 10^{23}\)

2) \(26 \times 10^{23}\)

3) \(34 \times 10^{23}\)

4) \(48 \times 10^{23}\) 159. The number of water molecules present in a drop of water (volume \(0.0018 \mathrm{~mL}\) ) at room temperature is

1) \(6.023 \times 10^{19}\)

2) \(1.084 \times 10^{18}\)

3) \(4.84 \times 10^{17}\)

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

160. One atom of an element \(X\) weight \(6.643 \times 10^{-23}\) g. number of moles of atom in \(20 \mathrm{~kg}\) is

1) 140

2) 150

3) 250

4) 500

161.Zinc sulphate contains \(22.65 \%\) of zinc and \(43.9 \%\) of water of crystallization. If the law of constant proportions is true then the weight of zinc required to produce \(20 \mathrm{~g}\) of the crystals will be

1) \(45.3 \mathrm{~g}\)

2) \(4.53 \mathrm{~g}\)

3) \(0.453 \mathrm{~g}\)

4) \(453 \mathrm{~g}\)

162. Out of \(1.0 \mathrm{~g}\) dioxygen, \(1.0 \mathrm{~g}\) (atomic) oxygen and \(1.0 \mathrm{~g}\) ozone, the maximum number of molecules are contained in

1) \(1.0 \mathrm{~g}\) of atomic

2) \(1.0 \mathrm{~g}\) of ozone oxygen

3) \(1.0 \mathrm{~g}\) of oxygen gas 4)All contain same number of atoms

163. \(n\) gram of a substance \(X\) reacts with \(m\) gram of substance \(Y\) to form \(p\) gram of substance \(R\) and \(q\) gram of substance \(S\). This reaction can be represented as follows

\(X+Y=R+S\)

The relation which can be established in the amounts of the reactants and the products will be

1) \(n-m=p-q\)

2) \(n+m=p+q\)

3) \(n=m\)

4) \(p=q\)

164. What volume of \(6 \mathrm{MHCL}\) should be added to 2 M HCL to get 1 L of 3 M HCL?

1) \(0.25 \mathrm{~L}\)

2) \(1.00 \mathrm{~L}\)

3) \(0.75 \mathrm{~L}\)

4) \(2.50 \mathrm{~L}\)

165. Carbon dioxide contains \(27.27 \%\) of carbon, carbon disulphide contains \(15.79 \%\) of carbon and sulphur dioxide contains \(50 \%\) of sulphur. This data is an agreement with

1) Law of conservation 2) Law of definite of mass proportions

3) Law of multiple

4) Law of reciprocal proportions proportions

166. Which of the following pairs contains equal number of atoms?

1) 11.2 cc (STP) of

2) \(22.4 \mathrm{~L}\) (STP) of nitrogen and \(0.015 \mathrm{~g}\) nitrous oxide and of nitric oxide \(\quad 22.4 \mathrm{~L}\) of nitric oxide 1 millimole of HCL 3) and 0.5 millimole of \(\mathrm{H}_{2} S\)

1 mole of \(\mathrm{H}_{2} \mathrm{O}_{2}\) and 1

4) mole of \(\mathrm{N}_{2} \mathrm{O}_{4}\)

167. Cortisone is a molecular substance containing 21 atoms of carbon per molecule. The molecular weight of cortisone is 360.4 . what is the percentage of carbon in cortisone?

1) \(59.9 \%\)

2) \(75 \%\)

3) \(69.98 \%\)

4) None of these

168. Choose the wrong statement.

1 mole means 6.023 2) Molar mass is mass

1) \(\times 10^{23}\) particles of one molecule

3) Molar mass is mass 4) Molar mass is of one mole of a molecular mass substance expressed in grams

169. If in a reaction \(\mathrm{HNO}_{3}\) is reduced to \(\mathrm{NO}\), the mass of \(\mathrm{HNO}_{3}\) absorbing one mole of electrons would be

1) \(21.0 \mathrm{~g}\)

2) \(36.5 \mathrm{~g}\)

3) \(18.0 \mathrm{~g}\)

4) \(31.5 \mathrm{~g}\)

170. Equal weights of \(\mathrm{Zn}\) metal and iodine are mixed together and \(l_{2}\) is completely converted to \(Z n l_{2}\). What fraction by weight of original \(\mathrm{Zn}\) remains unreacted? \((\mathrm{Zn}=65, \mathrm{I}=127)\)

1) 0.34

2) 0.74

3) 0.84

4) Unable to predict

171.If 0.5 mole of \(\mathrm{BaCl}_{2}\) is mixed with 0.2 mole of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\), the maximum number of moles \(\mathrm{f}\) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) that can be formed is

1) 0.7

2) 0.5

3) 0.03

4) 0.10

172.0n analysis a certain compound was found to contain iodine and oxygen in the ratio of \(254 \mathrm{~g}\) of iodine (at. mass 127) and \(80 \mathrm{~g}\) oxygen (at. mass 16). What is the formula of the compound?

1) \(I O\)

2) \(\mathrm{I}_{2} \mathrm{O}\)

3) \(\mathrm{I}_{2} \mathrm{O}_{3}\)

4) \(\mathrm{I}_{2} \mathrm{O}_{5}\)

173. Cyclohexanol is dehydrated to cyclohexene on heating with conc \(\mathrm{H}_{2} \mathrm{SO}_{4}\). The cyclohexene obtained from \(100 \mathrm{~g}\) cyclohexanol will be (If yield of reaction is \(75 \%\) )

1) \(61.5 \mathrm{~g}\)

2) \(75.0 \mathrm{~g}\)

3) \(20.0 \mathrm{~g}\)

4) \(41.0 \mathrm{~g}\)

174. One atom of an element weights \(1.8 \times 10^{-22} \mathrm{~g}\). its atomic mass is

1) 29.9

2) 18

3) 108.36

4) 154

175. In the following reaction, which choice has value twice that of the equivalent mass of the oxidizing agent?

\(\mathrm{SO}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow 3 \mathrm{~S}+2 \mathrm{H}_{2} \mathrm{O}\)

1) 64

2) 32

3) 16

4) 48 176. An organic compound contains \(20.0 \% \mathrm{C}, 6.66 \%\) \(\mathrm{H}, 47.33 \% \mathrm{~N}\) and the rest was oxygen. Its molar mass is \(60 \mathrm{~g} \mathrm{~mol}^{-1}\) the molecular formula of the compound is

1) \(\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}\)

2) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{NO}_{2}\)

3) \(\mathrm{CH}_{3} \mathrm{~N}_{2} \mathrm{O}\)

4) \(\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}_{2}\)

177. The reaction between yttrium metal, \(Y\) and dilute hydrochloric acid produces \(\mathrm{H}_{2}(g)\) and \(Y^{3+}\) icons. The molar ratio of yttrium used to hydrogen produces is

1) \(1: 2\)

2) \(1: 3\)

3) \(2: 1\)

4) \(2: 3\)

178. About a gaseous reaction, \(x X+y Y \rightarrow l L+m M\) Which statement is wrong?

\(x\) letre of \(X\) combines

\(x\) moles of \(X\)

1) with \(y\) litre of \(Y\) to give \(L\) and \(M\) 2) combines with \(y\) \(x\) number of molecules of \(X\) and \(M\)

3) combine with \(y\) \(x \mathrm{~g}\) of \(X\) combines number of molecules \(M\) and \(L\) of \(Y\) to form \(L\) and \(M\) 5)

179. Which property of an element is always a whole number?

1)Atomic volume

2) Atomic weight

3)Atomic number

4) Equivalent weight

180. Two elements \(X\) (at. Wt. 75) and \(Y\) (at. wt. 16) combine to give a compound having \(75.8 \%\) of \(X\) . The formula of compound will be

1) \(X Y\)

2) \(X_{2} Y\)

3) \(X Y_{3}\)

4) \(X_{2} Y_{3}\)

181. Insulin contains \(3.4 \%\) sulphur. What will be the minimum molecular weight of insulin?

1) 94.117

2) 1884

3) 941.176

4) 976

182. NO reacts with \(\mathrm{O}_{2}\) to form \(\mathrm{No}_{2}\). When \(10 \mathrm{~g}\) of \(\mathrm{NO}_{2}\) is formed during the reaction, the mass of \(\mathrm{O}_{2}\) consumed is

1) \(1.90 \mathrm{~g}\)

2) \(5.0 \mathrm{~g}\)

3) \(3.48 \mathrm{~g}\)

4) \(13.9 \mathrm{~g}\)

183. Arsenic forms two oxides, one of which contains \(65.2 \%\) and the other \(75.5 \%\) of the element. Hence, equivalent masses of arsenic are in the ratio

1) \(1: 2\)

2) \(3: 5\)

3) \(13: 15\)

4) \(2: 1\)

184. A metal oxide is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, \(3.15 \mathrm{~g}\) of oxide yielded \(1.05 \mathrm{~g}\) of metal. From the above data we can say that

1) The atomic weight of 2 ) The atomic weight of metal is 8 metal is 4

3) The equivalent

4) The equivalent weight of metal is 4 weight of metal is 8

185. The equivalent mass of chlorine is 35.5 and the atomic mass of copper is 63.5. the equivalent mass of copper chloride is 99.0 . hence, formula of copper chloride is

1) \(\mathrm{CuCl}\)

2) \(C u_{2} C l\)

3) \(\mathrm{CuCl}_{2}\)

4) None of these

186. In the following reaction, \(\mathrm{MnO}_{2}+4 \mathrm{HCL} \longrightarrow \mathrm{MnCl}_{2}+2 \mathrm{H}_{2} \mathrm{O}+\mathrm{Cl}_{2}\) \(2 \mathrm{~mol} \mathrm{MnO} \mathrm{M}_{2}\) reacts with \(4 \mathrm{~mol}\) of \(\mathrm{HCl}\) to form \(11.2 \mathrm{LCl}_{2}\) at STP. Thus, per cent yield of \(\mathrm{Cl}_{2}\) is

1) \(25 \%\)

2) \(50 \%\)

3) \(100 \%\)

4) \(75 \%\)

187.276 \(\mathrm{g}\) of silver carbonate on being strongly heated yields a residue weighing

1) \(3.54 \mathrm{~g}\)

2) \(3.0 \mathrm{~g}\)

3) \(1.36 \mathrm{~g}\)

4) \(2.16 \mathrm{~g}\)

188. An element, \(X\) has the following isotopic composition

\({ }^{200} X: 90 \%\)

\({ }^{199} X: 8.0 \%\)

\({ }^{202} X: 2.0 \%\)

The weighted average atomic mass of the naturally occurring element \(X\) is closed to

1) \(200 u\)

2) \(210 u\)

3) \(202 \mathrm{u}\)

4) \(199 u\)

189. For the reaction, \(X+2 Y \rightarrow Z\)

5 Moles of \(X\) and 9 moles of \(Y\) will produce

1) 5 moles of \(Z\)

2) 8 moles of \(Z\)

3) 14 moles of \(Z\)

4) 4 moles of \(Z\)

190. What is the number of moles of \(\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{~s})\) that can be produced by allowing 1 mole of \(\mathrm{Fe}_{2} \mathrm{~S}_{3^{3}}, 2\) moles of \(\mathrm{H}_{2} \mathrm{O}\) and 3 moles of \(\mathrm{O}_{2}\) to react as \(2 \mathrm{Fe}_{2} \mathrm{~S}_{3}+6 \mathrm{H}_{2} \mathrm{O}+3 \mathrm{O}_{2} \rightarrow 4 \mathrm{Fe}(\mathrm{OH})_{3}+6 \mathrm{~S}\) ?

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

2) \(1.84 \mathrm{~mol}\)

3) \(1.34 \mathrm{~mol}\)

4) \(1.29 \mathrm{~mol}\)

191.If \(w_{1}\) g of a metal \(X\) displaces \(w_{2} \mathrm{~g}\) of another metal \(Y\) from its salt solution and if the equivalent weights are \(E_{1}\) and \(E_{2}\) respectively, the correct expression for the equivalent weight of \(X\) is

1) \(E_{1}=\frac{w_{1}}{w_{2}} \times E_{2}\)

2) \(E_{1}=\frac{w_{2} \times E_{2}}{w_{1}}\) 

3) \(E_{1}=\frac{w_{1} \times w_{2}}{E_{2}}\)

4) \(E_{1}=\sqrt{\frac{w_{1}}{w_{2}} \times E_{2}}\)

192. The reaction of calcium with water is represented by the equation, \(\mathrm{Ca}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{H}_{2}\)

What volume of \(H_{2}\), at STP would be liberated when \(8 \mathrm{~g}\) of calcium completely reacts with water?

1) \(4480 \mathrm{~cm}^{3}\)

2) \(2240 \mathrm{~cm}^{3}\)

3) \(1120 \mathrm{~cm}^{3}\)

4) \(0.4 \mathrm{~cm}^{3}\)

193.100 \(\mathrm{mL}\) of \(0.1 \mathrm{~N}\) hypo decolourised iodine by the addition of \(x\) gram of crystalline copper sulphate to excess of KI. The value of ' \(x\) ' is (molecular wt. of \(\mathrm{CuSO}_{4}, 5 \mathrm{H}_{2} \mathrm{O}\) is 250)

1) \(5.0 \mathrm{~g}\)

2) \(1.25 \mathrm{~g}\)

3) \(2.5 \mathrm{~g}\)

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

194. Two oxides of a metal contain \(50 \%\) and \(40 \%\) metal \((M)\) respectively. If the formula of fist oxide is \(M O_{2}\), the formula of second oxide will be

1) \(M \mathrm{O}_{2}\)

2) \(\mathrm{MO}_{3}\)

3) \(M_{2} O\)

4) \(M_{2} O_{3}\)

195. In the reaction,

\(I_{2}+2 \mathrm{~S}_{2} \mathrm{O}_{3}^{2-} \rightarrow 2 I^{-}+\mathrm{S}_{4} \mathrm{O}_{6}^{2-}\)

Equivalent weight of iodine will be equal to \(\begin{array}{ll}\text { 1) Molecular weight } & \text { 2) } 1 / 2 \text { of molecular }\end{array}\) weight

3) \(1 / 4\) of molecular 4) Twice of molecular weight weight

196.100 tons of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) containing \(20 \%\) impurities will give iron by reduction with \(\mathrm{H}_{2}\) equal to

1) 112 tons

2) 80 tons

3) 160 tons

4) 56 tons

197. Haemoglobin contains \(0.33 \%\) of iron by weight. The molecular weight of haemoglobin is approximately 67200 . The number of iron atoms (at. Wt. of \(\mathrm{Fe}=56\) ) present in one molecule of haemoglobin is

1) 6

2) 1

3) 4

4) 2

198. In the final answer of the expression

\(\frac{(29.2-20.2)\left(1.79 \times 10^{5}\right)}{1.37}\), the number of significant figures is

1) 1

2) 2

3) 3

4) 4

199. The number of water molecules in \(1 \mathrm{~L}\) of water is

1) 18

2) \(18 \times 1000\)

3) \(N_{A}\)

4) \(55.55 N_{A}\)

200. The percentage of \(\mathrm{P}_{2} \mathrm{O}_{5}\) in diammonium hydrogen phosphate, \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) is

1) 23.48

2) 46.96

3) 53.78

4) 71.00