## Physical Chemistry Quiz | objective questions | Chemistry General Knowledge Questions | MCQ

**1 >>H combines with O to form two compounds, water and hydrogen peroxide. If 2 gm of H reacts with O completely to form 18 gm of water and 34 gm of hydrogen peroxide, then what is the ratio of mass of O combining with H? ?**

- (A)
**03:09** - (B)
**04:16** - (C)
**01:02** - (D) None of these

**2 >>The vapour density of a gas is 11.2, then 11.2 gm of this gas at NTP will occupy a volume of: ?**

- (A) 1.12 L
- (B) 0.112 L
- (C) 112 L
- (D) 11.2 L

**3 >>4 gm NaOH is present in 100 mL of its aqueous solution. What is the molarity? ?**

- (A) 2M
- (B) 1M
- (C) 10M
- (D) 0.1M

**4 >>The solution of H**

_{2}SO_{4}contains 80% by mass. Specific gravity of solution is 1.71 gm⁄cc. Find its molarity: ?- (A) 12
- (B) 13.95
- (C) 14
- (D) 17

**5 >>What is the weight percentage of NaCl solution in which 20 gm NaCl is dissolved in 60 gm of water? ?**

- (A) 0.1
- (B) 0.05
- (C) 0.25
- (D) 0.15

**6 >>A solution is prepared by mixing 10 mL of ethanol with 120 mL of methanol. What is the volume percentage of ethanol? ?**

- (A) 0.1
- (B) 0.077
- (C) 0.2
- (D) 0.15

**7 >>What is the weight by volume percentage of a solution in which 7.5 gm of KCl is dissolved in 100 mL of the solution? ?**

- (A) 0.075
- (B) 0.925
- (C) 0.5
- (D) None of these

**8 >>0.56 gm KOH is present in 100 mL of the solution. What is the normality? ?**

- (A) 1N
- (B) 0.1N
- (C) 2N
- (D) 0.2N

**9 >>Find the number of milli-equivalent of H**

_{2}SO_{4}present in 50 mL of N⁄20 H_{2}SO_{4}: ?- (A) 2.5
- (B) 1.5
- (C) 0.5
- (D) 2

**10 >>To prepare 600 mL of 2N solution of NH**

_{4}OH, what volume of 10N NH_{4}OH is required? ?- (A) 100 mL
- (B) 120 mL
- (C) 150 mL
- (D) 200 mL

**11 >>What volume of 2N and 5N H**

_{2}SO_{4}should be mixed so that the resultant solution of 1 L has N = 3? ?- (A) 1 mL
- (B) 0.5 mL
- (C) 0.75 mL
- (D) 1.5 mL

**12 >>Oxidation number of sulphur in Na**

_{2}S_{2}O_{3}is: ?- (A) 6
- (B) −2
- (C) −2 and +6
- (D) 2

**13 >>Equivalent weight of KMnO**

_{4}in alkaline medium is equal to: (M = molar mass) ?- (A) M
- (B) M⁄2
- (C) M⁄3
- (D) M⁄5

**14 >>Oxidation numbers of A, B and C are +6, −2 and −1 respectively. What will be the formula of the molecule when A, B and C associate with each other? ?**

- (A) AB
_{2}C_{2} - (B) ABC
_{2} - (C) AB
_{2}C - (D) A
_{2}BC

**15 >>Oxidation number of iodine in IO**

_{3}^{−}+ HI → H_{2}O + I_{2}: ?- (A) Increases
- (B) Decreases
- (C) Increases as well as decreases
- (D) Neither increases nor decreases

**16 >>In the presence of humidity, SO**

_{2}: ?- (A) Loses proton
- (B) Accepts electron
- (C) Is an oxidant
- (D) Is a reductant

**17 >>What will be the oxidation state of copper in YBa**

_{2}Cu_{3}O_{7}, if oxidation state of Y is +3? ?- (A) 7⁄3
- (B) 7
- (C) 3 and 5
- (D) None of these

**18 >>In the reaction, 3Br**

_{2}+ 6CO_{3}^{2−}+ 3H_{2}O → 5Br^{−}+ BrO_{3}^{−}+ 6HCO_{3}^{−}: ?- (A) Bromine is oxidised and carbonate is reduced
- (B) Bromine is reduced and water is oxidised
- (C) Bromine is neither reduced nor oxidised
- (D) Bromine is both reduced and oxidised

**19 >>The oxidation states of sulphur in Caro′s and Marshall′s acid are: ?**

- (A) +6, +6
- (B) +4, +6
- (C) +6, −6
- (D) +6, +4

**20 >>When methane is burnt in oxygen to produce CO**

_{2}and H_{2}O, the oxidation number changes by: ?- (A) −8
- (B) 0
- (C) 8
- (D) 4

**21 >>If the distance between Na**

^{+}and Cl^{−}ions in NaCl crystal is x pm, the length of the edge of unit cell is: ?- (A) x⁄2 pm
- (B) x⁄4 pm
- (C) 2x pm
- (D) 4x pm

**22 >>AB crystallizes in a body centered cubic lattice with edge length, a = 387 pm. The distance between two oppositely charged ions in the lattice is: ?**

- (A) 335 pm
- (B) 250 pm
- (C) 200 pm
- (D) 300 pm

**23 >>Fraction of total volume occupied by atoms in a simple cube is: ?**

- (A) π⁄2
- (B) √3π⁄2
- (C) √2π⁄6
- (D) π⁄6

**24 >>In a crystal, both ions are missing from normal sites in equal number. This is an example of: ?**

- (A) F−center
- (B) Interstitial defect
- (C) Frenkel defect
- (D) Schottky defect

**25 >>Xenon crystallizes in fcc lattice and the edge of the unit cell is 620 pm, then the radius of Xe atom is: ?**

- (A) 219.20 pm
- (B) 438.5 pm
- (C) 265.5 pm
- (D) 536.94 pm

**26 >>The edge length of cube is 400 pm. Its body diagonal would be: ?**

- (A) 500 pm
- (B) 693 pm
- (C) 600 pm
- (D) 566 pm

**27 >>The unit cell of a metallic element of atomic mass 10**

^{8}and density 10.5 gm⁄cm^{2}, is a cube with edge length of 409 pm. The structure of the crystal lattice is: ?- (A) fcc
- (B) bcc
- (C) hcp
- (D) None of these

**28 >>Copper metal has a fcc structure with a unit cell length of 0.361 nm. Picturing copper ions in contact along the face diagonal, the apparent radius of the copper ion is: ?**

- (A) 0.128
- (B) 1.42
- (C) 3.22
- (D) 4.22

**29 >>For an ionic crystal of the general formula AX and coordination number 6, the value of radius will be: ?**

- (A) In between 0.732 and 0.414
- (B) In between 0.414 and 0.225
- (C) Less than 0.225
- (D) Greater than 0.732

**30 >>The edge of unit cell of fcc Xe crystal is 620 pm. The radius of Xe atom is: ?**

- (A) 189.37 pm
- (B) 209.87 pm
- (C) 219.25 pm
- (D) 235.16 pm

**31 >>Which of the following statements is not true about NaCl structure? ?**

- (A) Cl
^{−}ions are in fcc arrangement - (B) Na
^{+}ions have coordination number 4 - (C) Cl
^{−}ions have coordination number 6 - (D) Each cell contains 4 NaCl molecules

**32 >>The ratio of cationic radius to anionic radius in an ionic crystal is greater than 0.732. Its coordination number is: ?**

- (A) 1
- (B) 4
- (C) 6
- (D) 8

**33 >>KF has NaCl sructure with edge length 537.5 x 10**

^{−12}m. What is the distance between K^{+}and F^{−}in KF, if density is 2.48 gm⁄cc? ?- (A) 268.8 pm
- (B) 19.415 x 10
^{−24}cc - (C) 134.4 pm
- (D) 19.415 x 10
^{−21}cc

**34 >>The number of atoms in 100 gm of a fcc crystal with density, d = 10 gm⁄cc and cell edge as 200 pm is equal to: ?**

- (A) 3 x 10
^{25} - (B) 5 x 10
^{24} - (C) 1 x 10
^{25} - (D) 2 x 10
^{25}

**35 >>TiO**

_{2}is a well known example of: ?- (A) Triclinic system
- (B) Tetragonal system
- (C) Monoclinic system
- (D) None of these

**36 >>Which one is correct about ferrites? ?**

- (A) They possess formula AB
_{2}O_{4}(A is divalent and B is trivalent cation) - (B) They possess spinel structure
- (C) MgAl
_{2}O_{4}is a ferrite - (D) All of the above

**37 >>Which of the following statements is true? ?**

- (A) Molecular crystals are very hard and incompressible
- (B) Ionic crystals have very low volatility
- (C) Metallic bond is directional and rigid
- (D) Boron nitride has an ionic crstal structure

**38 >>Graphite is a soft solid lubricant, extremely difficult to melt. The reason for this anomalous behaviour is that, graphite: ?**

- (A) Is a non−crystalline substance
- (B) Is an allotropic form of diamond
- (C) Has molecules of variable molecular masses like polymers
- (D) Has carbon atoms arranged in large plates of rings of strong bound carbon atoms with weak interplate bonds

**39 >>The appearance of colour in solid alkali metal halides is generally due to: ?**

- (A) Frenkel defect
- (B) Interstitial position
- (C) F−center
- (D) Schottky defect

**40 >>To 500 cc of water, 3 x 10**

^{−3}kg of acetic acid is added. If 23% of acetic acid is dissociated, what will be the depression in freezing point? K_{f}and density of water are 1.86 K⁄kg and 0.0997 gm⁄cc respectively. ?- (A) 0.186 K
- (B) 0.228 K
- (C) 0.371 K
- (D) 0.555 K

**41 >>A 0.1M solution of K**

_{2}SO_{4}is dissolved to the extent of 90%. What would be its osmotic pressure at 27^{o}C? ?- (A) 6.896 atm
- (B) 8.8 atm
- (C) 0.1 atm
- (D) None of these

**42 >>What is the value of i (Van′t Hoff factor) for phosphorus? ?**

- (A) 0.25
- (B) 0.5
- (C) 0.75
- (D) 1

**43 >>The vapour pressure of a liquid decreases by 10 torr when a non volatile solute is dissolved. The mole fraction of the solute in solution is 0.1. What will be the mole fraction of the liquid, if the decrease in the vapour pressure is 20 torr, the same solute being dissolved? ?**

- (A) 0.2
- (B) 0.9
- (C) 0.8
- (D) 0.6

**44 >>A 0.2M aqueous solution of a weak acid (HX) is 50% ionized. The freezing point of this solution is: (K**

_{f}= 1.86 kg⁄mol for water) ?- (A) −0.31
^{o}C - (B) −0.45
^{o}C - (C) −0.56
^{o}C - (D) −0.90
^{o}C

**45 >>If latent heat of fusion of ice is 80 cal⁄gm at 0**

^{o}C, calculate molal depression constant for water: ?- (A) 18.63
- (B) 186.3
- (C) 1.863
- (D) 0.1863

**46 >>Calculate the molal elevation constant of water that evaporates at 100**

^{o}C with the absorption of 536 cal⁄gm: (R = 2 cal) ?- (A) 0.519
^{o}C - (B) 0.0519
^{o}C - (C) 1.519
^{o}C - (D) 2.519
^{o}C

**47 >>15 gm of methyl alcohol is dissolved in 35 gm of water. What is the mass percentage of methyl alcohol in solution? ?**

- (A) 0.3
- (B) 0.5
- (C) 0.7
- (D) 0.75

**48 >>Osmotic pressure of a sugar solution at 24**

^{o}C is 2.5 atm. Determine the concentration of the solution in gm mol⁄L: ?- (A) 0.0821 mol⁄L
- (B) 1.082 mol⁄L
- (C) 0.1025 mol⁄L
- (D) 0.0827 mol⁄L

**49 >>0.15 gm of a substance, dissolved in 15 gm of solvent, was boiled at a temperature higher by 0.216**

^{o}C than that of the pure solvent. Calculate the molecular weight of the substance: (Molal elevation constant for the solvent = 2.16^{o}C) ?- (A) 216
- (B) 100
- (C) 178
- (D) None of these

**50 >>The relationship between osmotic pressure at 273 K when 10 gm glucose (P1), 10 gm urea (P2) and 10 gm sucrose (P3) are dissolved in 250 mL of water: ?**

- (A) P1 > P2 > P3
- (B) P3 > P2 > P1
- (C) P2 > P1 > P3
- (D) P2 > P3 > P1

**51 >>NaClO solution reacts with H**

_{2}SO_{3}as NaClO + H_{2}SO_{3}→ NaCl + H_{2}SO_{4}. A solution of NaClO used in this reaction contained 15 gm of NaClO per litre. The normality of the solution would be: ?- (A) 0.22
- (B) 0.33
- (C) 0.44
- (D) 0.55

**52 >>When mercuric iodide is added to the aqueous solution of potassium iodide, the: ?**

- (A) Freezing point is raised
- (B) Freezing point does not change
- (C) Freezing point is lowered
- (D) Boiling point does not change

**53 >>Benzene and toluene form nearly ideal solutions. At 20**

^{o}C, the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The partial vapour pressure of benzene at 20^{o}C for a solution containing 78 gm of benzene and 46 gm of toluene in torr is: ?- (A) 25
- (B) 50
- (C) 37.5
- (D) 53.5

**54 >>Two solutions of a substance are mixed in the following manner: 480 mL of 1.5M of solution 1 + 520 mL of 1.2M of solution 2. What is the molarity of the final mixture? ?**

- (A) 1.344M
- (B) 2.7M
- (C) 1.5M
- (D) 1.2M

**55 >>An aqueous solution of sucrose, containing 34.2 gm⁄L, has an osmotic pressure of 2.38 atm at 17**

^{o}C. For an aqueous solution of glucose to be isotonic with this solution, it would have: ?- (A) 18 gm⁄L
- (B) 16.2 gm⁄L
- (C) 36.6 gm⁄L
- (D) 14 gm⁄L

**56 >>0.01M solution of KCl nad BaCl**

_{2}are prepared in water. The freezing point of KCl is found to be −2^{o}C. What is the freezing point of BaCl_{2}solution, assuming both to be completely ionized? ?- (A) −3
^{o}C - (B) +3
^{o}C - (C) −2
^{o}C - (D) −4
^{o}C

**57 >>A 5% solution of sugarcane (mass = 342) is isotonic with 1% solution of X under similar conditions. The molecular weight of X is: ?**

- (A) 136.2
- (B) 68.4
- (C) 34.2
- (D) 171.2

**58 >>The use of anhydrous common salts is to clear snow on the roads. This causes: ?**

- (A) A lowering in freezing point of water
- (B) A lowering in melting point of ice
- (C) Ice melts at the temperature of the atmosphere present at that time
- (D) All of the above

**59 >>If a thin slice of suger beet is placed in concentrated solution of NaCl, then: ?**

- (A) Sugar beet will lose water from its cells
- (B) Sugar beet will absorb water from solution
- (C) Sugar beet will neither absorb nor lose water
- (D) Sugar beet will dissolve in solution

**60 >>Human blood has an osmotic pressure of 7.65 atm at body temperature. Hence, molarity of an intravenous glucose solution to have same osmotic pressure, will be: ?**

- (A) 0.3M
- (B) 0.1M
- (C) 0.5M
- (D) 0.2M