CHEMISTRY

Q1. X gmofa certainoxide ofnitrogenwasslowlypassed over heated copper to yield CuO and N2
gas. The
increase in the weight of copper was 5.33 gm 4 litre of N2
gas at 140
C and 754 mm of Hg was also
obtained. What is the formula ofthe oxide.
(A) N2
O5
(B) NO2
(C) NO (D) N2
O
Q2. CN–
is oxidised by NO3
–
in presence of acid :
aCN–
+ bNO3
–
+ cH+
 (a + b) NO + aCO2
+
c
2
H2
O
What are the values of a, b, c in that order.
(A) 3, 7, 7 (B) 3, 10, 10 (C) 3, 10, 7 (D) 3, 7, 10
Q3. One gram of Na3
AsO4
is boiled with excess ofsolid KI in presence ofstrong HCl. The iodine evolved
is absorbedin KI solutionandtitrated against 0.2 N hypo solution. Calculate thevolume ofthiosulphate
hypo used. (At. wt. ofAs = 75)
(A) 48.1 ml (B) 24.7 ml (C) 38.4 ml (D) 30.3 ml
Q4. How many grams of Zn of 90% purity would be needed to reduce 8.5 gm of NaNO3
in presence of
alkali. (At. wt. ofZn = 65.4)
(A) 32.2 gm (B) 19.8 gm (C) 29.1 gm (D) 23.11 gm
Q5. 7gm of a mixture of KClO3
and KCl are strongly heated, 2.50gm of O2
is produced. The residue on
analysis proves to be onlyKCl. Calculate the weight fractionofKClin the originalmixture.
(A) 0.0886 (B) 0.123 (C) 0.886 (D) 0.213
Q6. S2
O3
2–
ion is oxidised by S2
O8
2–
ion, the products are S4
O6
– –
and SO4
– –
ions. What volume of0.25 M
thiosulphate solution would be needed to reduce 1 gmofK2
S2
O8
.
(A) 36.92 ml (B) 32.69 ml (C) 29.63 ml (D) 62.93 ml
Q7. An element forms two different sulphates in which its weight % is 28 and 37. What is the ratio of
oxidation numbersofthe element inthese sulphates.
(A) 1 : 2 (B) 1 : 3 (C) 2 : 1 (D) 3 : 2
Q8. 12 gmurea (NH2
CONH2
) was treated with excess nitrous acid. The following reaction occurred.
NH2
CONH2
+ 2HNO2
 CO2
+ 2N2
+ 3H2
O
Thegasesevolvedwerepassed throughaqueousKOHsolutionandthe finalvolume ofthe remaininggas
was measured at STP. The volumeofthe remaining gas willbe
(A) 44.8 ml (B) 89.6 ml (C) 134.4 ml (D) 13.4 ml
Q9. The reaction betweenYttriummetaland dilute HClproduces H2
(g) andY3+
ions. The molar ratio ofY
used to hydrogen produced is
(A) 1 : 2 (B) 2 : 1 (C) 2 : 3 (D) 3 : 2
Q10. The number ofmoles of Cr2
O7
2–
needed to oxidize 0.136 equivalents ofN2
H5
+
bythe reaction is –
N2
H5
+
+ Cr2
I7
– –
 N2
+ Cr3+
+ H2
O
(A) 0.136 (B) 0.272 (C) 0.816 (D) 0.0227
Q11. The density of liquid ethanolis 0.7893 g/ml at 200
C. If1.2 mol ofethanol are needed for a particular
experiment, what volume ofethanolshouldbe measured out.
(A) 55 ml (B) 58 ml (C) 70 ml (D) 79 ml

Q12. A10gmsampleofamixtureofCalciumchlorideandsodiumchlorideistreatedwithNa2
CO3
to precipitate
the calciumas calciumcarbonate. WhenCaCO3
is ignited 1.62 gmCaO is obtained. The % bymass of
CaCl2
intheoriginalmixture is
(A) 15.2% (B) 32.1% (C) 21.8% (D) 11.07%
Q13. ThemolesofAmmoniumsulphate needed to react withone mole ofMnO2
inacidic mediuminareaction
giving MnSO4
and (NH4
)2
S2
O8
is
(A) 2 (B) 1/2 (C) 1 (D) 1/3
Q14. In a reaction FeS2
isoxidised byO2
to Fe2
O3
and SO2
. Iftheequivalent ofO2
consumed are X, then the
equivalents of Fe2
O3
and SO2
produced are
(A) X and X (B)
X
2
and X (C)
X
11
and
10
11
X
(D)
10
11
X
and
X
11
Q15. 100 mlof0.6 N H2
SO4
and 200 ml of0.3 N HCl were mixed together. The normality ofthe resulting
solutionwillbe
(A) 0.1N (B) 0.2N (C) 0.3N (D) 0.4N
Q16. 1g ofcarbonate of a metal was dissolved in 25ml ofN HCl. The resulting liquid required 5 mlof N -
NaOH for neutralization. The eq. wt. ofthe metalcarbonate is
(A) 50 (B) 30 (C) 20 (D) none
Q17. 5 ml ofN – HCl, 20 ml ofN/2 – H2
SO4
and 30mlof N/3 – HNO3
are mixed together and the volume
made to 1 litre.
(i) The normality of the resulting solution is
(A) N/5 (B) N/10 (C) N/20 (D) N/40
(ii) The wt. of pure NaOH required to neutralize the above solution is
(A) 10 g (B) 2 g (C) 1 g (D) 2.5 g
Q18. If0.5 molofBaCl2
is mixed with0.20 molofNa3
PO4
, the maximumamount of Ba3
(PO4
)2
that can be
formed is
(A) 0.70 mol (B) 0.50 mol (C) 0.20 mol (D) 0.10mol
Q19. The equivalent mass ofMnSO4
is halfofits molar mass when it is converted to
(A) Mn2
O3
(B) MnO2
(C) MnO4
–
(D) MnO4
2–
Q20. The anionnitratecanbe converted into ammoniumion. The equivalent mass ofNO3
–
ioninthis reaction
would be
(A) 6.20g (B) 7.75g (C) 10.5g (D) 21.0 g
Q21. The equivalent mass ofNa2
S2
O3
in its reaction with I2
is equalto
(A) molar mass (B)
molar mass
2
(C)
molar mass
3
(D)
molar mass
4
Q22. A solution ofKMnO4
is reduced to MnO2
. Thenormalityofsolutionis 0.6. The molarityis :
(A) 1.8 M (B) 0.6 M (C) 0.1M (D) 0.2 M
Q23. When one gramofKMnO4
reacts with HCl, the volume ofchlorine liberated at NTP willbe
(A) 11.2 litres (B) 22.4 litres (C) 44.8 litres (D) 56.0 litres

Q24. 8g of sulphur are burnt to formSO2
whichis oxidised byCl2
water. The solution is treated with BaCl2
solution. The amount ofBaSO4
precipitated is
(A) 1 mol (B) 0.5 mol (C) 0.24 mol (D) 0.25 mol
Q25. In an experiment 50 ml of 0.1M solution of a salt reacted with 25 ml of 0.1M solution of sodium
sulphite. The half equation for the oxidation of sulphite ion is:
SO3
2–
(aq.) + H2
O (l)  SO4
2–
(aq.) + 2H+
(aq.) + 2e–
If the oxidation number of metal in the salt was 3, what would be the new oxidation number of
metal?
(A) 0 (B) 1 (C) 2 (D) 4
Q26. WhenBrO3
–
ionreacts withBr–
ionin acidsolutionBr2
is liberated. Theequivalent weight ofKBrO3
in
this reactionis
(A) M/8 (B) M/3 (C) M/5 (D) M/6
where M is its molar mass.
Q27. Hydrogenperoxideinaqueoussolutiondecomposesonwarmingto giveoxygenaccordingto theequation
2H2
O2
(aq.)  2H2
O(l) + O2
(g) under conditions where one mole ofgas occupies 24 dm3
, 100cm3
of X M solution of H2
O2
produces 3 dm3
ofO2
X is thus
(A) 2.5 (B) 1 (C) 0.5 (D) 0.25
Q28. One mole of a mixture of CO and CO2
requires exactly20 grams of NaOH in solution for complete
conversion of all the CO2
into Na2
CO3
. How many extra grams of NaOH would it require for
conversion into Na2
CO3
ifthe mixture (one mole) is completelyoxidized to CO2
(A) 60 grams (B) 80 grams (C) 40 grams (D) 20 grams
Q29. Asolutioncontaining bothNa2
CO3
and NaHCO3
was treatedwithexcess ofCaCl2
solutionand filtered.
The precipitate weighed m1
grams. On adding NaOH indrops to the filtrate avoiding excess, a further
m2
grams was precipitated. If after adding excess CaCl2
, the solution (had not beenfiltered but) was
simplyboiled and thenfiltered, what would be the totalweight ofthe precipitate?
(A) (m1
+ m2
) grams (B) m
m
1
2
2






 grams
(C)
m m
1 2
2






 grams (D) m
m
2
1
2






 grams
Q30. One gram of a mixture of Na2
CO3
and NaHCO3
consumes y gram equivalents of HCl for complete
neutralization. One gram of the mixture is strongly heated, then cooled and the residue treated
withHCl. How manygrams equivalents ofHClwould be required for complete neutralization?
(A) 2 ygramequivalent (B) ygramequivalents
(C) 3y/4gramequivalents (D) 3y/2gramequivalents
Q31. Theoxidationstates ofthemost electronegative element inthe productsofthe reaction, BaO2
withdilute
H2
SO4
are
(A) 0 and –1 (B) –1 and –2 (C) –2 and 0 (D) –2 and +1
Q32. A solution contains Na2
CO3
and NaHCO3
. 10ml of the solution required 2.5 ml of 0.1M H2
SO4
for
neutralization usingphenolphthaleinas indicator. Methylorange is then addedwhen a further 2.5mlof
0.2 M H2
SO4
was required. The amount ofNa2
CO3
and NaHCO3
in1 litre ofthe solution is
(A) 5.3 g & 4.2g (B) 3.3 g & 6.2 g (C) 4.2 g & 5.3g (D) 6.2 g & 3.3 g

Q33. 0.5g offumingH2
SO4
(Oleum)isdilutedwithwater.Thissolutioniscompletelyneutralized by26.7mlof
0.4 N NaOH. The percentage of free SO3
in the sample is
(A) 30.6% (B) 40.6% (C) 20.6% (D) 50%
Q34. 34g ofhydrogenperoxide is present in1120 mlofsolution. This solution is called
(A) 10volsolution (B) 20volsolution (C) 30 volsolution (D) 32volsolution
Q35. A2g sampleofxenonreacts withfluorine. The mass ofthe compound produced is3.158g. The empirical
formula ofthe compound is
(A) XeF2
(B) XeF4
(C) XeF5
(D) XeF6
Q36. In which ofthe following redoxreaction‘n’factor ofeveryreactant is nonfractional
(A) CsBr + Br2
 CsBr3
(B) Mn3
O4
 Mn++
(C) KI + I2
 KI3
(D) NaNH2
+ N2
O  NaN3
+ H2
O
Q37. For 1.34 x 10–3
moles of KBrO3
to reduce into bromide 4.02 x 10–3
mole of Xn+
ion is needed. New
oxidationstate ofX is
(A) n + 2 (B) n – 2 (C) 2 (D) –2
Q38. The iodide content ofa solutionwas determined bytitration withcerium(IV) sulfate inthe presence of
HCl, in which I–
is converted to ICI. A250 ml sample of the solution required 20ml of 0.05 N Ce4+
solution. What is the iodide concentrationinthe originalsolution, ing/litre
(A) 0.254 g/lit (B) 2.54 g/lit (C) 0.508 g/lit (D) 5.08 g/lit
Q39. 0.218g ofanalkaline earth metalwhendissolved in dilute HClevolved 218.2 cc ofhydrogen at 170
C
and 754.4 mmcollected over water. Tension of aqueous vapour at 170
C = 14.4 mm. The equivalent
weight ofmetalis
(A) 12.22 (B) 24.22 (C) 23.93 (D) 11.96
Q40. 1 mole ofFe2
S3
, 2 moles ofH2
O and 3 moles of O2
are allowed to react according to the equation
2Fe2
S3
(s) + 6H2
O(l) + 3O2
(g)  4Fe(OH)3
(s) + 6S(s)
The number ofmoles ofFe(OH)3
(s) that canbe produced is
(A) 1.34 (B) 2 (C) 4 (D) 3
Q41. The equivalent weight ofCl2
inthe following two reactions are
MnO2
+ 4HCl  MnCl2
+ Cl2
+ 2H2
O
6NaOH + 3Cl2
 5NaCl + NaClO3
+ 3H2
O
(A) 35.5 & 35.5 (B) 35.5 & 71 (C) 35.5 & 14.2 (D) 35.5 & 42.6
Q42. 0.3 g ofa sample of an oxalate salt is dissolved in 100cc ofwater. It required 90 cc of N/20 KMnO4
solution for complete oxidation. The percentage ofoxalate (C2
O4
2–
) inthe givensample is
(A) 66 (B) 33 (C) 68 (D) 64
Q43. Two acids(A) and (B) are titrated separatelyeach timewith25 mlof1N Na2
CO3
solutionand required
10mland 40mlrespectivelyforcompleteneutralization. The volumes ofacid (A) and (B)require tomix
to produce one litre of1N acidsolution are respectively,
(A) 200 mlof (A) and 800 ml of(B) (B) 800 mlof (A) and 200 mlof(B)
(C) 400 mlof(A) and 400 ml of (B) (D) 600 mlof(A) and 400 ml of(B)

Q44. In a reaction, Cu2
S is oxidized byreacting with oxygen to give Cu2+
and SO2
. Ifthe equivalents ofO2
used were x, the equivalents of Cu2+
and SO2
produced w.r.t. Cu2
S would be
(A) xand x (B) x and 0.25 x (C) 0.25x and 0.75 (D) 0.75xand 0.25x
Q45. Whenthose compoundsare used as reducing agents, the equivalent weight ofKHC2
O4
, H2
C2
O4
·2H2
O
each is
(A) the sameas its molecular weight (B) halfofits molecular weight
(C) 1/4 of its molecular weight (D) 1/8 of its molecular weight
Q46. A hydrate ofiron(III) thiocynate, Fe(SCN)3
was foundto contain 19% H2
O. The empiricalformula of
the hydrate is
(A) Fe(SCN)3
·H2
O (B) Fe(SCN)3
·2H2
O (C) Fe(SCN)3
·3H2
O (D) Fe(SCN)3
·4H2
O
Q47. Manganese forms non-stoichiometric oxide having the general formula MnOx
. The value of x for a
compound that contained 63.7% Mn, is
(A) 2.08 (B) 1.958 (C) 1.858 (D) 2.18
Q48. A sample, supposed to be pure CaCO3
, is used to standardize a solution of HCl. The substance was
actually a mixture of MgCO3
and BaCO3
, but the standardization was corect in spite of erroneous
assumption. The percentage ofMgCO3
inthe mixture would be
(A)30.2% (B) 72.1% (C) 27.9% (D) 69.8%
Q49. An oleum sample containing 40% SO3
is diluted with sufficient H2
O. The % labelling of this oleum
sample would be
(A) 105% (B) 107% (C) 109% (D) 111%
Q50. 6 equivalent ofFeC2
O4
ontreatment with 2 mole of K2
Cr2
O7
inacidic mediumevolves x litre ofCO2
gas at STP. The value ofx would be
(A) 22.4 l (B) 44.8 l (C) 67.2 l (D) 89.6 l