Percentage composition Questions - Shailendra Kumar Chemistry
Percentage composition Questions - Shailendra Kumar Chemistry
Percentage composition Questions - Shailendra Kumar Chemistry
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PHYSICAL CHEMISTRY<br />
By: <strong>Shailendra</strong> <strong>Kumar</strong><br />
1. An organic substance gave on analysis the following percentage <strong>composition</strong>, C = 60%,<br />
H = 6.4%, N = 10.1%, O = 23.5%. The empirical formula of the compound is :<br />
(a) C 6<br />
H 8<br />
NO 2<br />
(b) C 6<br />
H 5<br />
NO 2<br />
(c) C 7<br />
H 9<br />
NO 2<br />
(d) C 7<br />
H 10<br />
NO 2<br />
2. An organic compound has the following percentage <strong>composition</strong>, C = 40% H = 6.7%,<br />
and O = 53.3%. The empirical formula of the compound is :<br />
(a) CH 2<br />
O (b) CHO<br />
(c) CHO 3<br />
(d) C 2<br />
H 2<br />
O 2<br />
3. 0.30 g of an organic substance on combustion gave 0.66 g of carbon dioxide and 0.36<br />
g of water. Its V.D. is 30. The molecular formula is :<br />
(a) C 3<br />
H 8<br />
O (b) C 2<br />
H 4<br />
O 2<br />
(c) C 8<br />
H 3<br />
O 2<br />
(d) C 4<br />
H 4<br />
O<br />
4. An organic compound on analysis gave the following results :<br />
C = 65%, H = 3.5%, N = 9.6%, O = 21.9%<br />
0.365 g if the substance displaced in a Victor Meyer’s apparatus 56 mL of dry air at<br />
S.T.P. The molecular formula of the substance is :<br />
(a) C 8<br />
H 5<br />
NO 2<br />
(b) C 4<br />
H 5<br />
NO 2<br />
2<br />
(c) C 6<br />
H 5<br />
N 2<br />
O 2<br />
(d) C 4<br />
H 6<br />
N 4<br />
O 4<br />
5. A compound contains the following percentage of elements :- C = 12.76, H = 2.13 and<br />
Br = 85.11. Its vapour density is 95. Its molecular formula is :<br />
(a) CH 3<br />
Br (b) C 2<br />
H 4<br />
Br 2<br />
(c) C 3<br />
H 6<br />
Br 2<br />
(d) C 4<br />
H 4<br />
Br 4<br />
6. The empirical formula of a compound is CH 2<br />
. 0.083 mole of the compound contains 2.0<br />
g of carbon, the molecular formula of the compound is :<br />
(a) C 4<br />
H 8<br />
(b) C 3<br />
H 6<br />
(c) C 2<br />
H 4<br />
(d) C 2<br />
H 2<br />
7. 0.1 mole of a compound of S and Cl on oxidation with conc. HNO 3<br />
and subsequent<br />
treatment gave 0.1 mole of PbCl 2<br />
and 0.2 mole of BaSO 4<br />
as precipitates. The molecular<br />
formula of the compound is :<br />
(a) SCl (b) S 2<br />
Cl 2<br />
(c) SCl 4<br />
(d) SCl 3<br />
8. Two elements A (at.wt. = 12) and B (at. wt. = 16) combine to yield a compound. The<br />
percentage by weight of A in the compound is 27.3 %. The formula of the compound will<br />
be :<br />
(a) A 2<br />
B 2<br />
(b) AB<br />
(c) A 2<br />
B (d) AB 2<br />
9. On analysis of an organic compound the following results were obtained :<br />
C = 31.9%, H = 6.8%, N = 18.5%<br />
The empirical formula of the compound is :<br />
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2. House no. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna<br />
Page No.: 1
PHYSICAL CHEMISTRY<br />
1. Opp. Khuda Baksh Library, Ashok Rajpath, Patna - 4<br />
2. House no. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna<br />
By: <strong>Shailendra</strong> <strong>Kumar</strong><br />
(a) C 2<br />
H 5<br />
NO (b) CH 3<br />
NO 2<br />
(c) C 2<br />
H 4<br />
N (d) C 2<br />
H 5<br />
NO 2<br />
10. 0.0833 mole of the carbohydrate (empirical formula CH 2<br />
O) contains 1.00 g of hydrogen.<br />
The molecular formula of the carbohydrate is :<br />
(a) C 6<br />
H 12<br />
O 6<br />
(b) C 5<br />
H 10<br />
O 5<br />
(c) C 2<br />
H 5<br />
N (d) C 2<br />
H 5<br />
NO 2<br />
11. 0.220 g of an organic compound gave upon analysis 0.6179 g of CO 2<br />
and 0.124 g of<br />
H 2<br />
O. The empirical formula of the compound is :<br />
(a) C 6<br />
H 6<br />
O 2<br />
(b) C 5<br />
H 6<br />
O 2<br />
(c) C 6<br />
H 6<br />
O (d) C 6<br />
H 4<br />
O 3<br />
12. A gaseous compound of carbon and nitrogen containing 53.8 percent by weight of<br />
nitrogen was found to have a vapour density of 25.8. The molecular formula of the<br />
compound is :<br />
(a) CN (b) C 2<br />
N 2<br />
(c) CN 2<br />
(d) C 2<br />
N 3<br />
13. The percentage of oxygen in heavy water is :<br />
(a) 80 (b) 60<br />
(c) 88.9 (d) 50<br />
14. 0.2154 g of an organic compound gave on combustion 0.4308 g of CO 2<br />
and 0.1766 g of<br />
H 2<br />
O. The vapour density of the compound is 44. The molecular formula of the compound<br />
is :<br />
(a) C 2<br />
H 2<br />
O (b) C 4<br />
H 8<br />
O 2<br />
(c) C 3<br />
H 4<br />
O 3<br />
(d) C 2<br />
H 2<br />
O 2<br />
15. A quantity of 2.40 g of the oxide of a metal X (atomic mass = 55.9 a.m.u) was heated<br />
in carbon monoxide. The mass of the metal formed is 1.68 g. The simplest formula of<br />
the oxide is :<br />
(a) XO (b) X 2<br />
O<br />
(c) X 2<br />
O 3<br />
(d) XO 2<br />
16. 64 g of an organic compound consisting of carbon, hydrogen and oxygen contains in<br />
the ratio 3 : 1 : 4 by weight, respectively. The empirical formula of the compound is (a)<br />
CH 2<br />
O (b) C 2<br />
H 4<br />
O<br />
(c) C 2<br />
H 6<br />
O 2<br />
(d) CH 4<br />
O<br />
17. An organic compound containing C, H and O is found to have 32% C, 4% H, the<br />
remaining being oxygen. The molecular formula of the compound if it contains six<br />
atoms of oxygen per molecule is :<br />
(a) C 2<br />
H 2<br />
O 6<br />
(b) C 4<br />
H 6<br />
O 6<br />
(c) C 6<br />
H 6<br />
O 6<br />
(d) C 3<br />
H 6<br />
O 6<br />
18. A compound contains 28% nitrogen and 72% metal by mass. 3 atoms of the metal<br />
combine with 2 atoms of nitrogen. The atomic mass of the metal is :<br />
(a) 23 (b) 24<br />
(c) 39 (d) 40<br />
Page No.: 2
PHYSICAL CHEMISTRY<br />
By: <strong>Shailendra</strong> <strong>Kumar</strong><br />
19. A substance on analysis gave the following percentage <strong>composition</strong> : Na = 27.38%, H =<br />
1.19%, C = 14.28%, O = 57.14%. The empirical formula of the compound is :<br />
(a) NaHC 3<br />
(b) Na 2<br />
CO 3<br />
(c) Na 2<br />
CO 3<br />
.10 H 2<br />
O (d) Na 2<br />
CO 3<br />
.7 H 2<br />
O<br />
20. Three of the following formulae might be either empirical or molecular formula but one<br />
of the four must be a molecular formula. The one is :<br />
(a) N 2<br />
O (b) N 2<br />
O 4<br />
(c) NH 3<br />
(d) Mg 3<br />
N 2<br />
21. A gas is found to have the formula (CO)n. Its vapour density is 70. The value of n will be<br />
:<br />
(a) 1 (b) 2 (e) 5<br />
(c) 3 (d) 4<br />
22. A gaseous compound contains carbon and hydrogen in atomic ratio 1 : 2. 0.32 g of<br />
oxygen and 0.42 g of the conpound occupies the same volume under similar conditions<br />
of temperature and pressure. The molecular formula of the compound is :<br />
(a) C 2<br />
H 4<br />
(b) C 3<br />
H 6<br />
(c) C 4<br />
H 8<br />
(d) C 5<br />
H 10<br />
23. The compound C 7<br />
H 7<br />
NO 2<br />
:<br />
(a) contains 17 atoms per mole<br />
(b) contains equal percentage of C and H by weight<br />
(c) contains twice the percent by mass of oxygen as of nitrogen<br />
(d) contains twice the percent by mass of nitrogen as of hydrogen<br />
24. A compound consisting of only carbon and chlorine shows on analysis 10.15% carbon<br />
and 89.85% chlorine . If each molecule weighs 3.93 x 10 –22 g, the molecular formula of<br />
the compound would be :<br />
(a) CCl 4<br />
(b) C 2<br />
Cl 6<br />
(c) C 2<br />
Cl 4<br />
(d) C 2<br />
Cl 2<br />
25. 10 g of hydrofluric acid occupies 5.60 litres at S.T.P. The empirical formula of the gas<br />
is HF, the molecular formula in gaseous state will be :<br />
(a) HF (b) H 2<br />
F 2<br />
(c) H 3<br />
F 3<br />
(d) H 4<br />
F 4<br />
26. The elements A (at.wt. = 75) and B (at. wt. = 25) combine to yield a compound. The % by<br />
weight of A in the compound was found to be 75.0. The formula of the compound is :<br />
(a) AB (b) AB 2<br />
(c) A 2<br />
B 2<br />
(d) A 2<br />
B<br />
27. The formula which represents the simple ratio of atoms is :<br />
(a) molecular formula<br />
(b) structureal formula<br />
(c) empirical formula<br />
(d) rational formula<br />
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2. House no. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna<br />
Page No.: 3
PHYSICAL CHEMISTRY<br />
By: <strong>Shailendra</strong> <strong>Kumar</strong><br />
28. A 24.00 g sample of an oxide of iron contains 6.63 g of oxygen. The simplest formula of<br />
the compound (Fe = 56) would be :<br />
(a) Fe 3<br />
O 4<br />
(b) FeO<br />
(c) Fe 2<br />
O 3<br />
(d) Fe 4<br />
O 6<br />
29. Atomic <strong>composition</strong> of entire universe is approximately 93% hydrogen and 7% helium.<br />
The percentage by weight of hydrogen is :<br />
(a) 72.8 (b) 76.8 (c) 93 (d) 95.8<br />
30. A sample of hydrocarbon on combustion gave 7.92 g of CO 2<br />
and 3.24 g of water. The<br />
weight of the sample that was burnt was :<br />
(a) 2.52 g (b) 2.0 g<br />
(c) 1.52 g (d) 1.0 g<br />
31. The relative number of atoms in a hydrocarbon is C = 0.75 and H =3. The empirical<br />
formula of the hydrocarbon is :<br />
(a) C 3<br />
H 8<br />
(b) C 2<br />
H 6<br />
(c) CH 4<br />
(d) none<br />
32. The empirical formula of an organic compound containing carbon and hydrogen is<br />
CH 2<br />
. The mass of 1.0 L of this compound is exactly equal to that of 1.0 L of N 2<br />
under<br />
identical conditions. The molecular formula of the hydrocarbon is :<br />
(a) C 2<br />
H 4<br />
(b) C 3<br />
H 6<br />
(c) C 6<br />
H 12<br />
(d) C 4<br />
H 8<br />
33. An organic compound has empirical formula CH 2<br />
O and its molecular weight is 90. Its<br />
molecular formula is :<br />
(a) C 2<br />
H 4<br />
O (b) C 3<br />
H 4<br />
O 3<br />
(c) C 3<br />
H 6<br />
O 3<br />
(d) C 2<br />
H 4<br />
O 2<br />
34. Molecular weight of a compound is 180. 0.0833 mole of the compound contains 5 g of<br />
carbon. The molecular formula of the compound is :<br />
(a) C 5<br />
H 10<br />
O 5<br />
(b) C 9<br />
H 8<br />
O 4<br />
(c) C 5<br />
H 8<br />
O 7<br />
(d) C 10<br />
H 12<br />
O 3<br />
35. The empirical formula of the compound containing 50% of element A (atomic weight<br />
10) and 50% of element B (at.wt.20) is :<br />
(a) AB (b) A 2<br />
B<br />
(c) AB 2<br />
(d) A 2<br />
B 2<br />
36. An organic compound contians x% C, y% H, and z% O. If x =6y and (x-y) = 3 (z-y), the<br />
empirical formula of the compound is :<br />
(a) CH 2<br />
O (b) CHO<br />
(c) C 3<br />
H 8<br />
O 3<br />
(d) C 3<br />
H 6<br />
O<br />
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Page No.: 4