The document contains questions related to mole concept and stoichiometry calculations. It asks the reader to calculate quantities like number of moles, atoms, molecules, and mass involved in various chemical reactions and substances. It also contains matching questions to test the reader's understanding of stoichiometric relationships between reactants and products in chemical equations.

1. Topic – Mole Concept
1. Calculate number of neutrons present in 12 x 1025 atoms of oxygen (8O17):
(Given: NA= 6x1023)
(a) 1800
(b) 1600
(c) 1800 NA
(d) 3200 NA
2. If mass of one atom is 3.32 x 10-23 g, then calculate number of number of nucleons (neutrons
and protons ) present in 2 atoms of the element:
(a) 40
(b) 20
(c) 10
(d) 40 NA
3. Calculate number of electrons present in 9.5 g of P𝑂4
3−
:
(a) 6
(b) 50NA
(c) 0.1NA
(d) 4.7 NA
4. What is the number of moles of O- atom in 126 amuof HNO3?
(a) 2
(b)
2
N
A
(c) 6
(d)
6
𝑁𝑎
5. Total no. of electrons present in 48 g. Mg 2+are:
(a) 24 N A
(b) 2 N A
(c) 20 N A
(d) None of these
6. 3.011 x 1022 atoms of an element weight 1.15 gm. The atomic mass of the element is:
(a) 10 amu
(b) 2.3 amu

2. (c) 35.5 amu
(d) 23 amu
7. Cisplatin, an anticancer drug, has the molecular formula Pt (NH3)2Cl2. What is the mass ( in
gram) of one molecule? (atomic weights: pt = 195, H= 1.0, N = 14, Cl = 35.5)
(a) 4.98 x10-21
(b) 4.98 x10-22
(c) 6.55 x10-21
(d) 3.85 x10-22
8. The number of gram – molecule of oxygen which are contained in 6.02 x 1024 CO
molecules is
(a) 10 g molecule
(b) 5 g molecule
(c) 1 g molecule
(d) 0.5 g molecule
9. The mass of 1 x 1022 molecules of CuSO4. 5H2O is
(a) 41.59 g
(b) 415.9 g
(c) 4. 159 g
(d) None of these
10. The weight of one molecule of a compound C60H122 is
(a) 1.2 x 10-20gm
(b) 1.4 x 10-21gm
(c) 5.025 1023gm
(d) 6.023 1023gm
11. Number of atoms in 4.25 g of ammonia approximately
(a) 6 x 1023
(b) 15 x 1023
(c) 1.5 x 1023
(d) 2.5 x1023
12. The number of molecules in 4.25 gm of ammonia is
(a) 1.5 x 1023
(b) 2.5 x1023
(c) 3.5 x 1023

3. (d) 15 x 1023
13. The weight of an atom of oxygen is
(a) 026.557 x 1023g
(b) 26.556 x 1023g
(c) 2.656 x 10-23g
(d) 4. 538 x 10-23g
14. How many water molecules are there in one drop of water ( volume 0.0018 ml) at room
temperature:
(a) 4.86 x 1017
(b) 6.023 x 1024
(c) 2.584 x 1019
(d) 6.023 x 1019
15. The weight of one molecule of a compound C60H122 is
(a) 1.3 x 10-20 g
(b) 5.01 x 10-21 g
(c) 3.72 x 1023 g
(d) 1.4 x 10-21 g
16. Volume occupied by one molecule of water (density = 1 g cm-3 ) is
(a) 3.0 x 10-23 cm3
(b) 5.5 x 10-23 cm3
(c) 9.0 x 10-23 cm3
(d) 6.023 x 10-23 cm3
17. In a gaseous reaction of the type, aA + bB → cC + dD, which statement is wrong?
(a) A litres of A combine with b litres of B to give C and D
(b) A moles of A combine with b moles of B to give Product
(c) A g of A combine with b g of B to give C and D
(d) A molecules of A combine with b molecules of B to give C and D
18. The equation 2Al (s) +
3
2
O2 (g) → Al2O3(s) shows that
(a) 2 moles of Al react with
3
2
moles of O2to produce
7
2
moles of Al2O3
(b) 2 g of Al react with
3
2
g of O2 to produce one mole of Al2O3
(c) 2 g of Al react with
3
2
litres of O2to produce 1 mole of Al2O3
(d) 2 moles of Al react with
3
2
moles of O2to produce 1 mole of Al2O3

4. 19. If 5 litres of H2O2produce 50 litres of O2at NTP, H2O2 is
(a) ‘50V’
(b) ‘10V’
(c) ‘5V’
(d) ‘250V’
20. 2.76g silver carbonate on being strongly heated yields a residue weighing
(a) .00216Kg
(b) .00218Kg
(c) 2.12g
(d) 2.14g
21. Assuming that petrol is octane (C8H18) and has density 0.8 g /mL, 1.425 litres of petrol on
complete combustion will consume
(a) 50 moles of O2
(b) 100 moles of O2
(c) 125 moles of O2
(d) 200 moles of O2
22. 12 g of Mg will react completely with an acid to give
(a) 1 mole of O2
(b)
1
2
mole of H2
(c) 1 mole of H2
(d) 2 moles of H2
23. 10 mL of gaseous hydrocarbon on combustion gives 40 mL of CO2(g) and 50 mL of H2O
(vap). The hydrocarbon is
(a) C4H5
(b) C8H10
(c) C4H8
(d) C4H10
24. For complete oxidation of 4 liters of CO at NTP, the required volume of O2at NTP
(a) 4 litres
(b) 8 litres
(c) 2 litres
(d) 1 litre
25. The minimum quantity in grams of H2S needed to precipitate 63.5 g of Cu2+ will be nearly
(a) 63.5 g

5. (b) 31.75 g
(c) 34 g
(d) 20 g
26. If 0.5 mole of BaCl2is mixed with 0.2 mole of Na3PO4, the maximum number of mole of
Ba3(PO2)2 that can be formed is
(a) 0.7
(b) 0.5
(c) 0.30
(d) 0.1
27. For the reaction A + 2B → C, 5 moles of A and 8 moles of B will produce
(a) 5 moles of C
(b) 4 moles of C
(c) 8 moles of C
(d) 13 moles of C
Match the column
28.
Column-I Column-II
(a) Compound containing 5 g S and 5 g
oxygen atom
(p) Empirical formula CH2
(b) Hydrocarbon contain
800
11
% C (q) Molecular formula
C2H4
(c)
300
11
% of C and
800
11
of O (r) Empirical formula SO2
(d) Hydrocarbon containing
100
7
% H (s) Empirical formula CO2
29.
Column-I
(Amount of substance )
Column-II
(No. of moles of particular
atoms in the given substance )
(a) 6. 022 x 1024 molecules of
Al2(SO4)3. 3H2O
(p) 15 mole O- atoms
(b) 90 gm C6H12O6 (q) 60 mole H- atoms
(c) 112 litre So3(g) at 1 atm and 00C (r) 3 mole O-atoms
(d) 3.75 mole N2O4 (s) 30 mole S- atoms
(t) 150 mole O- atoms

6. 30.
Column-I Column-II
(a) 120 g CH3COOH in 1 L solution dsol =
1.2 g/ mL
(p) M=2
(b) 120 g glucose dissolved in 1 L
solution dsol = 1.2 g/mL
(q) 10% w/w sol.
(C) X NH2CONH2 =
1
31
(aqucous- solution ) (r) 12 % w/v sol.
(c) 19.6 % (w/v)H2SO4solution → (dsol =
1.2 g/mL)
(s) m= 1.85
31.
Column-I Column-II
(a) 1 M glucose solution (p) 1 mol solute per litre solution
(b) 3 M urea solution (q) 180 g solute per litre solution
(c) 3 M CH3COOH solution (r) % w/v = 18% (solution)
(d) 1 M H2SO4 soution (s) % w/v = 9.8% (solution)
32.
Column-I Column-II
(a) 49 g H2SO4 (p) 0.5 mole
(b) 20 g NaOH (q) 1.5 NA atoms
(c) 11.35 L of CO2 at STP (r) 0.5 NA molecule
(d) 6.022 x 1023 atoms of oxygen (s) 2 mole of O atom
33.

7. Column-I
Fur 1 mole of reactant placed in
open container in such reaction
Column-II
Product
(c) PCl5 (g) PCl3(g) + Cl2(g) (p) 2NA molecules
(d) CaCO3(s) CaO(s) + CO2(g) (q) 68.1 litre gaseous product at
STP
(e) 2HCl(g) H2(g) + Cl2 (r) 22.7 litre gaseous product at
STP
(f) NH4COONH3(s) 2NH3 +
CO2(g)
(s) 45.4 litre gaseous product at
STP
34.
Column-I Column-II
(a) 32 g each of O2and S (p) 2 moles of Fe
(b) 2 gram – molecule of K3[Fe(CN)6] (q) 3 moles of ozone
molecule
(c) 144 g of oxygen atom (r) one mole
(d) From 168 g of iron, 6.022 x1023 atoms
of iron are removed, the iron left
(s) 12 mole of carbon atoms
Answer Key Match the column
Column-I Column-II
(e) Compound containing 5 g S and 5 g
oxygen atom R
(p) Empirical formula CH2
(f) Hydrocarbon contain
800
11
% C p (q) Molecular formula
C2H4
(g)
300
11
% of C and
800
11
of O S (r) Empirical formula SO2
(h) Hydrocarbon containing
100
7
% H PQ (s) Empirical formula CO2
Column-I
(Amount of substance )
Column-II
(No. of moles of particular
atoms in the given substance )

8. (e) 6. 022 x 1024 molecules of
Al2(SO4)3. 3H2O QTS
(p) 15 mole O- atoms
(f) 90 gm C6H12O6 R (q) 60 mole H- atoms
(g) 112 litre So3(g) at 1 atm and 00C
P
(r) 3 mole O-atoms
(h) 3.75 mole N2O4 P (s) 30 mole S- atoms
(t) 150 mole O- atoms
Column-I Column-II
(d) 120 g CH3COOH in 1 L solution dsol =
1.2 g/ mLpqrs
(p) M=2
(e) 120 g glucose dissolved in 1 L
solution dsol = 1.2 g/mLqR
(q) 10% w/w sol.
(C) X NH2CONH2 =
1
31
(aqucous- solution )
SQ
(r) 12 % w/v sol.
(f) 19.6 % (w/v)H2SO4solution → (dsol =
1.2 g/mL) P
(s) m= 1.85
Column-I Column-II
(e) 1 M glucose solution PQR (p) 1 mol solute per litre solution
(f) 3 M urea solution Q R (q) 180 g solute per litre solution
(g) 3 M CH3COOH solution
QR
(r) % w/v = 18% (solution)
(h) 1 M H2SO4 soution P S (s) % w/v = 9.8% (solution)

9. Column-I Column-II
(b) 49 g H2SO4 PSR (p) 0.5 mole
(b) 20 g NaOH PQR (q) 1.5 NA atoms
(e) 11.35 L of CO2 at STP P R
Q
(r) 0.5 NA molecule
(f) 6.022 x 1023 atoms of oxygen
R
(s) 2 mole of O atom
Column-I
Fur 1 mole of reactant placed in
open container in such reaction
Column-II
Product
(g) PCl5 (g) PCl3(g) + Cl2(g) PS (p) 2NA molecules
(h) CaCO3(s) CaO(s) + CO2(g) PR (q) 68.1 litre gaseous product at
STP
(i) 2HCl(g) H2(g) + Cl2
R
(r) 22.7 litre gaseous product at
STP
(j) NH4COONH3(s) 2NH3 +
CO2(g) Q
(s) 45.4 litre gaseous product at
STP
Column-I Column-II
(e) 32 g each of O2and S R (p) 2 moles of Fe
(f) 2 gram – molecule of K3[Fe(CN)6] PS (q) 3 moles of ozone
molecule
(g) 144 g of oxygen atom Q (r) one mole
(h) From 168 g of iron, 6.022 x1023 atoms
of iron are removed, the iron left P
(s) 12 mole of carbon atoms