Chemistry Arithmetic PDF Past Paper

13. In known elements, the maximum number is of [CPMT 1985] (a) Metals...

13. In known elements, the maximum number is of [CPMT 1985] (a) Metals (b) Non-metals (c) Metalloids (d) None of these 14. Which one of the following is not an element (a) Diamond (b) Graphite Significant figures, Units for measurement, (c) Silica (d) Ozone Matter and Separation of mixture 15. A mixture of ZnCl 2 and PbCl 2 can be separated by 1. One fermi is [Haryana CEET 1994; DPMT 2004] [AFMC 1989] (a) Distillation (b) Crystallization (a) 10 13 cm (b) 10 15 cm (c) Sublimation (d) Adding aceitic acid (c) 10 10 cm (d) 10 12 cm 16. A mixture of methyl alcohol and acetone can be separated by 2. A picometre is written as (a) Distillation (a) 10 9 m (b) 10 10 m (b) Fractional distillation (c) 10 11 m (d) 10 12 m (c) Steam distillation 3. One atmosphere is equal to (d) Distillation under reduced pressure (a) 101.325 K pa (b) 1013.25 K pa 17. In the final answer of the expression (29.2  20.2) (1.79  10 5 ) (c) 10 5 Nm (d) None of these. The number of significant figures 1.37 4. Dimensions of pressure are same as that of is [CBSE PMT 1994] [CBSE PMT 1995] (a) 1 (b) 2 (a) Energy (b) Force (c) 3 (d) 4 (c) Energy per unit volume (d) Force per unit volume 18. 81.4 g sample of ethyl alcohol contains 0.002 g of water. The 5. The prefix 1018 is [Kerala MEE 2002] amount of pure ethyl alcohol to the proper number of (a) Giga (b) Nano significant figures is (c) Mega (d) Exa (a) 81.398 g (b) 71.40 g 6. Given the numbers : 161cm, 0.161cm, 0.0161 cm. The number (c) 91.4 g (d) 81 g of significant figures for the three numbers are 19. The unit J Pa 1 is equivalent to [CBSE PMT 1998] (a) m 3 (b) cm 3 (a) 3, 4 and 5 respectively (b) 3, 3 and 3 respectively (c) 3, 3 and 4 respectively (d) 3, 4 and 4 respectively (c) dm 3 (d) None of these 7. Significant figures in 0.00051 are 20. From the following masses, the one which is expressed nearest to the milligram is (a) 5 (b) 3 (a) 16 g (b) 16.4 g (c) 2 (d) 4 (c) 16.428 g (d) 16.4284 g 8. Which of the following halogen can be purified by sublimation [Manipal PMT 2001] 21. The number of significant figures in 6.02  10 23 is (a) F2 (b) Cl 2 (a) 23 (b) 3 (c) Br2 (d) I2 (c) 4 (d) 26 9. Difference in density is the basis of [Kerala MEE 2002] 22. The prefix zepto stands for [DPMT 2004] (a) Ultrafiltration (b) Molecular sieving (a) 10 9 (b) 10 12 (c) Gravity Separation (d) Molecular attraction (c) 10 15 (d) 10 21 10. Which of the following elements of matter would best convey 23. The significant figures in 3400 are [BHU 2004] that there is life on earth (a) 2 (b) 5 (a) Oxygen (b) Hydrogen (c) 6 (d) 4 (c) Carbon (d) Iron 24. The number of significant figures in 6.0023 are 11. The compound which is added to table salt for maintaining [Pb.CET 2001] proper health is (a) 5 (b) 4 (a) KCl (b) KBr (c) 3 (d) 1 (c) NaI (d) MgBr2 25. Given P  0.0030m , Q  2.40m , R  3000m , Significant 12. Which of the following contains only one element figures in P, Q and R are respectively [Pb. CET 2002] (a) Marble (b) Diamond (a) 2, 2, 1 (b) 2, 3, 4 (c) Glass (d) Sand (c) 4, 2, 1 (d) 4, 2, 3 26. The number of significant figures in 60.0001 is 9. Two elements X and Y have atomic weights of 14 and 16. They [Pb. CET 2000] form a series of compounds A, B, C, D and E in which the same (a) 5 (b) 6 amount of element X, Y is present in the ratio 1 : 2 : 3 : 4 : 5. If (c) 3 (d) 2 the compound A has 28 parts by weight of X and 16 parts by weight of Y, then the compound of C will have 28 parts weight 27. A sample was weighted using two different balances. The of X and [NCERT 1971] result’s were (i) 3.929 g (ii) 4.0 g. How would the weight of the sample be reported (a) 32 parts by weight of Y (b) 48 parts by weight of Y (a) 3.929 g (b) 3 g (c) 64 parts by weight of Y (d) 80 parts by weight of Y (c) 3.9 g (d) 3.93 g 10. Carbon and oxygen combine to form two oxides, carbon monoxide and carbon dioxide in which the ratio of the weights Laws of chemical combination of carbon and oxygen is respectively 12 : 16 and 12 : 32. These figures illustrate the 1. Which of the following pairs of substances illustrate the law of (a) Law of multiple proportions multiple proportions [CPMT 1972, 78] (b) Law of reciprocal proportions (a) CO and CO2 (b) H 2 O and D2 O (c) Law of conservation of mass (c) NaCl and NaBr (d) MgO and Mg(OH ) 2 (d) Law of constant proportions 11. A sample of calcium carbonate (CaCO 3 ) has the following 2. 1.0 g of an oxide of A contained 0.5 g of A. 4.0 g of another oxide of A contained 1.6 g of A. The data indicate the law of percentage composition : Ca = 40%; C = 12%; O = 48% (a) Reciprocal proportions (b) Constant proportions If the law of constant proportions is true, then the weight of calcium in 4 g of a sample of calcium carbonate obtained from (c) Conservation of energy (d) Multiple proportions another source will be 3. Among the following pairs of compounds, the one that (a) 0.016 g (b) 0.16 g illustrates the law of multiple proportions is (c) 1.6 g (d) 16 g (a) NH 3 and NCl 3 (b) H 2 S and SO 2 12. n g of substance X reacts with m g of substance Y to form p g of (c) CuO and Cu 2 O (d) CS 2 and FeSO 4 substance R and q g of substance S. This reaction can be represented as, X  Y  R  S. The relation which can be 4. The percentage of copper and oxygen in samples of CuO established in the amounts of the reactants and the products will be obtained by different methods were found to be the same. This (a) n  m  p  q (b) n  m  p  q illustrates the law of [AMU 1982, 92] (c) n  m (d) pq (a) Constant proportions (b) Conservation of mass (c) Multiple proportions (d) Reciprocal proportions 13. Which of the following is the best example of law of conservation of mass [NCERT 1975] 5. Two samples of lead oxide were separately reduced to metallic lead by heating in a current of hydrogen. The weight of lead (a) 12 g of carbon combines with 32 g of oxygen to form 44 g from one oxide was half the weight of lead obtained from the of CO 2 other oxide. The data illustrates [AMU 1983] (b) When 12 g of carbon is heated in a vacuum there is no (a) Law of reciprocal proportions change in mass (b) Law of constant proportions (c) A sample of air increases in volume when heated at (c) Law of multiple proportions constant pressure but its mass remains unaltered (d) Law of equivalent proportions (d) The weight of a piece of platinum is the same before and 6. Chemical equation is balanced according to the law of after heating in air [AMU 1984] 14. The law of multiple proportions is illustrated by the two (a) Multiple proportion (b) Reciprocal proportion compounds [NCERT 1972] (c) Conservation of mass (d) Definite proportions (a) Sodium chloride and sodium bromide 7. Avogadro number is (b) Ordinary water and heavy water (a) Number of atoms in one gram of element (c) Caustic soda and caustic potash (b) Number of millilitres which one mole of a gaseous (d) Sulphur dioxide and sulphur trioxide substances occupies at NTP 15. In compound A, 1.00 g nitrogen unites with 0.57 g oxygen. In (c) Number of molecules present in one gram molecular mass compound B, 2.00 g nitrogen combines with 2.24 g oxygen. In of a substance compound C, 3.00 g nitrogen combines with 5.11 g oxygen. (d) All of these These results obey the following law [CPMT 1971] 8. Different propartions of oxygen in the various oxides of (a) Law of constant proportion nitrogen prove the [MP PMT 1985] (b) Law of multiple proportion (a) Equivalent proportion (b) Multiple proportion (c) Law of reciprocal proportion (c) Constant proportion (d) Conservation of matter (d) Dalton's law of partial pressure 16. Hydrogen combines with oxygen to form H 2 O in which 16 g 4. 1 amu is equal to of oxygen combine with 2 g of hydrogen. Hydrogen also 1 1 (a) of C  12 (b) of O - 16 combines with carbon to form CH 4 in which 2 g of hydrogen 12 14 combine with 6 g of carbon. If carbon and oxygen combine (c) 1g of H 2 (d) 1.66  10 23 kg together then they will do show in the ratio of 5. Sulphur forms the chlorides S 2 Cl 2 and SCl 2. The equivalent (a) 6 : 16 or 12 : 32 (b) 6 : 18 mass of sulphur in SCl 2 is (c) 1 : 2 (d) 12 : 24 17. 2 g of hydrogen combine with 16 g of oxygen to form water [EAMCET 1985; Pb. CET 2001] and with 6 g of carbon to form methane. In carbon dioxide 12 g (a) 8 g/mole (b) 16 g/mole of carbon are combined with 32 g of oxygen. These figures (c) 64.8 g/mole (d) 32 g/mole illustrate the law of 6. The sulphate of a metal M contains 9.87% of M. This sulphate (a) Multiple proportions (b) Constant proportions is isomorphous with ZnSO 4.7 H 2 O. The atomic weight of M (c) Reciprocal proportions (d) Conservation of mass is [IIT 1991] 18. An element forms two oxides containing respectively 53.33 and (a) 40.3 (b) 36.3 36.36 percent of oxygen. These figures illustrate the law of (c) 24.3 (d) 11.3 (a) Conservation of mass (b) Constant proportions 7. When 100 ml of 1 M NaOH solution and 10 ml of (c) Reciprocal proportions (d) Multiple proportions 10 N H 2 SO 4 solution are mixed together, the resulting solution 19. After a chemical reaction, the total mass of reactants and will be [DPMT 1982] products [MP PMT 1989] (a) Alkaline (b) Acidic (a) Is always increased (b) Is always decreased (c) Strongly acidic (d) Neutral (c) Is not changed (d) Is always less or more 8. In chemical scale, the relative mass of the isotopic mixture of 20. A sample of pure carbon dioxide, irrespective of its source oxygen atoms (O 16 , O 17 , O 18 ) is assumed to be equal to contains 27.27% carbon and 72.73% oxygen. The data support [AIIMS 1992] [Bihar MADT 1981] (a) Law of constant composition (a) 16.002 (b) 16.00 (c) 17.00 (d) 11.00 (b) Law of conservation of mass 9. For preparing 0.1 N solution of a compound from its impure (c) Law of reciprocal proportions sample of which the percentage purity is known, the weight of (d) Law of multiple proportions the substance required will be [MP PET 1996] 21. The law of definite proportions is not applicable to nitrogen (a) More than the theoretical weight oxide because [EAMCET 1981] (b) Less than the theoretical weight (a) Nitrogen atomic weight is not constant (c) Same as the theoretical weight (b) Nitrogen molecular weight is variable (d) None of these (c) Nitrogen equivalent weight is variable 10. 1 mol of CH 4 contains (d) Oxygen atomic weight is variable (a) 6.02  10 23 atoms of H 22. Which one of the following pairs of compounds illustrates the law of multiple proportion [EAMCET 1989] (b) 4 g atom of Hydrogen (a) H 2O, Na 2O (b) MgO, Na 2O (c) 1.81  10 23 molecules of CH 4 (d) 3.0 g of carbon (c) Na 2O, BaO (d) SnCl 2 , SnCl 4 11. In the reaction 2 Na2 S 2O3  I2 Na2 S 4 O6  2 NaI , the Atomic, Molecular and Equivalent masses equivalent weight of Na 2 S 2 O 3 (mol. wt. = M) is equal to (a) M (b) M / 2 1. Which property of an element is always a whole number (c) M / 3 (d) M / 4 [MP PMT 1986] 12. When potassium permanganate is titrated against ferrous (a) Atomic weight (b) Equivalent weight ammonium sulphate, the equivalent weight of potassium (c) Atomic number (d) Atomic volume permanganate is [CPMT 1988] 2. Which one of the following properties of an element is not (a) Molecular weight /10 (b) Molecular weight /5 variable [Bihar MADT 1981] (c) Molecular weight /2 (d) Molecular weight (a) Valency (b) Atomic weight 13. Boron has two stable isotopes, 10 B (19%) and 11 B (81%). The (c) Equivalent weight (d) All of these atomic mass that should appear for boron in the periodic table 3. The modern atomic weight scale is based on is [CBSE PMT 1990] [MP PMT 2002] (a) 10.8 (b) 10.2 12 16 (a) C (b) O (c) 11.2 (d) 10.0 (c) H1 (d) C 13 14. What is the concentration of nitrate ions if equal volumes of 0.1 27. The atomic weights of two elements A and B are 40 and 80 M AgNO 3 and 0.1 M NaCl are mixed together respectively. If x g of A contains y atoms, how many atoms are [CPMT 1983; NCERT 1985] present in 2x g of B (a) 0.1 M (b) 0.2 M y y (a) (b) (c) 0.05 M (d) 0.25 M 2 4 15. Total number of atoms represented by the compound (c) y (d) 2y CuSO4.5H2O is [BHU 2005] 28. Assuming fully decomposed, the volume of CO 2 released at (a) 27 (b) 21 (c) 5 (d) 8 STP on heating 9.85g of BaCO 3 (Atomic mass of Ba=137) 16. 74.5 g of a metallic chloride contain 35.5 g of chlorine. The will be [CBSE PMT 2000] equivalent weight of the metal is [CPMT 1986] (a) 0.84 L (b) 2.24 L (a) 19.5 (b) 35.5 (c) 4.06 L (d) 1.12 L (c) 39.0 (d) 78.0 29. If N A is Avogadro’s number then number of valence electrons 17. 7.5 grams of a gas occupy 5.8 litres of volume at STP the gas is (a) NO (b) N 2 O in 4.2 g of nitride ions ( N 3 ) (c) CO (d) CO 2 (a) 2.4 N A (b) 4.2 N A 18. The number of atoms in 4.25 g of NH 3 is approximately (c) 1.6 N A (d) 3.2 N A [CBSE PMT 1999; MH CET 2003] 30. The weight of 1  10 22 molecules of CuSO 4.5 H 2 O is (a) 1  10 23 (b) 2  10 23 [IIT 1991] (c) 4  10 23 (d) 6  10 23 (a) 41.59 g (b) 415.9 g 19. One litre of a gas at STP weight 1.16 g it can possible be (c) 4.159 g (d) None of these [AMU 1992] 31. Rearrange the following (I to IV) in the order of increasing (a) C2 H 2 (b) CO masses and choose the correct answer from (a), (b), (c) and (d) (c) O2 (d) CH 4 (Atomic mass: N=14, O=16, Cu=63). 20. The vapour density of a gas is 11.2. The volume occupied by I. 1 molecule of oxygen 11.2 g of the gas at ATP will be [Bihar CET 1995] II. 1 atom of nitrogen (a) 11.2 L (b) 22.4 L (c) 1 L (d) 44.8 L III. 1  10 10 g molecular weight of oxygen 21. Equivalent weight of crystalline oxalic acid is IV. 1  10 10 g atomic weight of copper [MP PMT 1995] (a) 30 (b) 63 (a) II