Chemistry

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CAREER POINT PRE FOUNDATION DIVISION SUMMER WORKSHOP (IJSO) Daily Practice Problem Sheet Subject : Chemistry

Topic : Mole Concept

DPPS. NO. – 01 .

OBJECTIVE TYPE QUESTIONS : Q.1

Rearrange the following (I to IV) in the order of increasing masses. (I) 0.5mole of O3 (II) 0.5 gm molecule of Nitrogen 23 (III) 3.011 × 10 molecules of O2 (IV) 11.35 L of CO2 at STP. (A) IV < III < II < I (B) II < III < IV < I (C) III < II < I < IV (D) I < II < III < IV

Q.2

A mixture of gas ''X'' (mol.wt. 16) and gas "Y" (mol. wt. 28) in the mole ratio a : b has a mean molecular weight 20. What would be mean molecular weight if the gases are mixed in the ratio b : a under identical conditions (gases are non reacting). (A) 24 (B) 20 (C) 26 (D) 40

Q.3

The percentage by mole of NO2 in a mixture of NO2(g) and NO(g) having average molecular mass 34 is : (A) 25% (B) 20% (C) 40% (D) 75%

Q.4

An iodized salt contains 0.5% of NaI. A person consumes 3 gm of salt everyday. The number of iodide ions going into his body everyday is (A) 10–4 (B) 6.02 ×10–4 (C) 6.02 × 1019 (D) 6.02 × 1023

Q.5

Which has the maximum number of atoms ? (A) 24 g C (12) (B) 56 g Fe (56)

(C) 27 g Al (27)

(D) 108 g Ag (108)

Q.6

A 5.2 molal aqueous solution of methyl alcohol, CH3OH, is supplied. What is the mole fraction of methyl alcohol in the solution ? (A) 0.100 (B) 0.190 (C) 0.086 (D) 0.050

Q.7

The molarity of a solution obtained by mixing 750mL of 0.5 (M) HCl with 250 mL of 2 (M) HCl will be : (A) 1.00M (B) 1.75M (C) 0.975M (D) 0.875M

Q.8

A gaseous hydrocarbon gives upon combustion 0.72 g of water and 3.08 g of CO2. The empirical formula of the hydrocarbon is : (A) C3H4 (B) C6H5 (C) C7H8 (D) C2H4

Q.9

One mole of oxalic acid is equivalent to (A) 0.5 mole of NaOH (C) 1.5 mole of NaOH

(B) 1 mole of NaOH (D) 2 mole of NaOH

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Q.10

When 1g of CaCO3 reacts with 50 ml of 0.1 M HCI, the volume of CO2 produced is (A) 11.2 mL (B) 22.4 mL (C) 112 mL (D) 56 mL

Q.11

How many H atoms are in 3.4 g of C12H22O11 ? (A) 6.0 × 1023 (B) 1.3 × 1023

(C) 3.8 × 1022

(D) 6.0 × 1024

Q.12

How many atoms are contained in a mole of Ca(OH)2 (A) 30 × 6.02 × 1023 atoms/mol (B) 5 × 6.02 × 1023 atoms/mol (C) 6 × 6.02 × 1023 atoms/mol (D) None of these

Q.13

Equivalent mass of KMnO4, when it is converted to MnSO4 is (A) M/5 (B) M/3 (C) M/6

Q.14

Sulphur trioxide is prepared by the following two reactions S8(s) + 8O2(g)  8SO2(g) 2SO2(g) + O2(g)  2SO3(g) How many grams of SO3 are produced from 1 mole of S8 ? (A) 1280 (B) 640 (C) 960

Q.15

(D) M/2

(D) 320

In a compound AxBy (A) Mole of A = Mole of B = mole of AxBy (B) Eq. of A = Eq. of B = Eq. of AxBy (C) X × mole of A = y × mole of B = (x + y) × mole of AxBy (D) X × mole of A = y × mole of B


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Topic : Structure of Atom

DPPS. NO. – 02 .


The element having electronic configuration [Kr] 4d134f145s25p65d1 6s2 belongs to – (A) s–block (B) p–block (C) d–block (D) f–block

Q.2

The designation of an orbital with n=4 and =3 is – (A) 4s (B) 4p (C) 4f

Q.3

Q.4

(D) 4d

The sets of quantum numbers for an electron in 4f orbital is – (A) n = 4,  = 3, m = + 1, s = + ½

(B) n = 4,  = 4, m = – 4, s = – ½

(C) n = 4,  = 3, m = + 4, s = + ½

(D) n = 3,  = 2, m = – 2, s = + ½

The following ions that has the maximum magentic moment is – (A) Mn2+ (B) Fe2+ (C) Ti2+

(D) Cr2+

Q.5

Degenerate orbitals means – (A) Orbitals having equal energy (B) Orbitals having equal wave function (C) Orbitals having equal energy but different wave function (D) Orbitals having equal energy and equal wave function

Q.6

Heisenberg's uncertainty principle is applicable to – (A) atoms only (B) electron only (C) nucleus only (D) any fast moving sub atomic particle

Q.7

The e/m ratio of the anode rays depend upon – (A) Nature of residual gas (C) Nature of discharge tube

(B) Nature of electrode (D) Nature of anode

Penetration power of proton is (A) Greater than electron (C) Greater than neutron

(B) Less than electron (D) It cannot penetrate

Q.8

Q.9

The ground state electronic configuration of Cr is – (A) [Ar]3d4 4s1 (B) [Ne]3d5 4s1 (C) [Ne]3d4 4s1


(D) [Ar]3d5 4s1

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Q.10

Q.11

The ratio of radii of third and first Bohr orbital of hydrogen atom is – (A) 4:1 (B) 1:4 (C) 1:9

(D) 9:1

A f-sub shell can accommodate to a maximum of – (A) 2 electrons (B) 6 electrons (C) 10 electrons

(D) 14 electrons

Q.12

The energy of a radiation of wavelength 4000Å is E1 and that of radiation of 8000 Å is E2. E1 and E2 are related as (A) E1= E2 (B) E1= 3E2 (C) 3E1= E2 (D) E1= 2E2

Q.13

Example of isosters is – (A) CO2 and CO (B) CO2 and N2O

(C) CO2 and NO

(D) NO and NO2

Q.14

Presence of three unpaired electrons in phosphorus atom can be explained by – (A) Pauli's rule (B) Hund's rule (C) uncertainty principle (D) Aufbau's rule

Q.15

How much energy in kJ is produced when 7.1 g of gaseous chlorine atoms are converted to gaseous chloride ions ? (Electron affinity of chlorine is -3.7eV). (1eV/atm = 96.49 kJ/moles) (A) 35.7 kJ (B) 26.2 kJ (C) 68.5 kJ (D) 71.4 kJ

Q.16

The orbital diagram in which the Hund’s rule is violated is (A) (B) (C)

Q.17

Q.18

The p-orbitals have (A) dumb-bell shape (C) double dumb bell shape

(D)

(B) spherical shape (D) complex structure

Pick out the isoelectronic structures from the following  CH3+ H3O+   NH3  (A)  and  (B)  and V (C)  and 

V CH3– (D) , , V

Q.19

The atomic orbital is (A) the circular path of the electron. (B) elliptical shaped orbit. (C) three dimensional field around nucleus. (D) the region in which there is maximum probability of finding an electron.

Q.20

The last electron of the element of atomic number 31 will have the following quantum numbers n  m s (A) 3 0 0 –1/2 (B) 3 1 1 +1/2 (C) 4 1 –1 –1/2 (D) 4 0 0 +1/2


Page # 2



Topic : Chemical Equlibrium

DPPS. NO. – 03 .


One of the favourable conditions for the backward reaction is – (A) increase in the concentration of the reactant (B) the removal of atleast one of the products at regular intervals (C) increase in the concentration of one or more product (D) increase in the volume of container

Q.2

An acidic buffer solution can be prepared by mixing the solution of – (A) sodium acetate and acetic acid (B) ammonium chloride and ammonium hydroxide (C) sulphuric acid and sodium hydroxide (D) sodium chloride and sodium hydroxide

Q.3

When pressure is applied to the equilibrium system, Ice water (A) more ice is formed (B) water is evaporated (C) more water is formed (D) equilibrium is not formed

Q.4

The reaction will shift towards the product side, when the I2(g) 2I(g), H = + 150 kJ (A) concentration of I2 is decreased (B) concentration of I is increased (C) temperature is increased (D) total pressure is increased

Q.5

Equilibrium constant for the reaction 2NO(g) + Cl2(g) 2NOCl(g) is correctly given by the expression2 [2 NOCl] [ NOCl] [ NOCl]2 [ NOCl]2 (A) K  (B) K  (C) K  (D) K  2 2 2 [2 NO][Cl 2 ] [ NO] [Cl 2 ] [ NO] [Cl 2 ] [ NO]2  [Cl 2 ]

Q.6

For a reversible reaction, if the concentrations of the reactants are doubled, the equilibrium constant will be – (A) doubled (B) same (C) halved (D) one fourth

Q.7

Consider the following reaction, K1 K2 H2SO4 H+ + HSO4– ; HSO4– H+ + SO42– The equilibrium constant K for the following dissociation is H2SO4 (A) k1 + k2 (B) k1k2 (C) k1 k2

Q.8

The reaction will be favoured by 2SO2 + 2O2 2SO3 + 193.2 kJ (A) high temperature and low pressure (C) low temperature and high pressure

2H+ + SO42– (D) k1 – k2

(B) high temperature and high pressure (D) low temperature and low pressure

Q.9

The pH of a solution is increased from 3 to 6; its H+ ion concentration will be – (A) reduced to half (B) doubled (C) reduced by 1000 times (D) increased by 1000 times

Q.10

According to Lewis concept, an acid is – (A) an electron pair donor (C) an electron pair acceptor

(B) proton donor (D) proton acceptor


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Q.11

When H2 and I2 are mixed and equilibrium is attained, then (A) amount of HI formed is equal to the amount of H2 dissociated (B) HI dissociation stops (C) the reaction stops completely (D) none of these

Q.12

Minimum dissociation constant among the following is shown by – (A) CHCl2COOH (B) CH2ClCOOH (C) CH3COOH

Q.13

1 O2 2 respectively. The relationship between K1 and K2 is -

The equilibrium constant of equilibrium SO2 +

(A) K2 = 2 K1

(B) K2 = K12

(C) K2 =

SO3 1 K1

(D) CCl3COOH

and 2SO2 + O2

(D) K2 =

2SO3 are K1 and K2 1 K12

Q.14

When two reactants A and B are mixed to give products C and D, the reaction quotient, Q, at the initial stage of the reaction – (A) is zero (B) decreases with time (C) is independent of time (D) increases with time

Q.15

Consider the reaction CaCO3(s) CaO(s) + CO2(g) in closed container at equilibrium. What would be the effect of addition of CaCO3 on the equilibrium concentration of CO2 ? (A) Increases (B) Decreases (C) Data is not sufficient to predict it (D) Remains unaffected.

Q.16

The value of equilibrium constant for an unfavourable forward reaction is (A) less than one (B) equal to one (C) more than one (D) None of these

Q.17

When NH4Cl is added to NH4OH solution, the dissociation of ammonium hydroxide is reduced. It is due to (A) common ion effect (B) hydrolysis (C) oxidation (D) reduction

Q.18

Which of the following will change the value of the equilibrium constant for the reaction? N2(g) + O2(g)  2NO (g) (A) Add more N2 (B) Increase of pressure (C) Use a smaller reaction vessel (D) Increase the temperature

Q.19

Variation of the concentration of the reactant (X) and the product (Y) are shown in the figure. Select the correct statement.

(A) I and II both are kinetic regions. (C) I is equilibrium and II is kinetic region. Q.20

(B) I and II both are equilibrium regions. (D) I is kinetic and II is equilibrium region.

At 5 atm pressure PCl5 gas dissociates by 10%. What will be the value of Kp at same temperature ? (A) 0.045 atm (B) 0.050 atm (C) 0.9 atm (D) 0.5 atm


Page # 2



Topic : Acids, Bases & Salts

DPPS. NO. – 04 .


Efflorescence is shown during – (A) crystallization of washing soda (B) loss of some molecules of water of crystallization (C) formation of anhydrous sodium carbonate (D) cleansing action of washing soda

Q.2

Addition of water to an acid is avoided because – (A) The reaction is endothermic (B) The reaction is exothermic (C) The acid will get diluted (D) The acid will loose its properties

Q.3

Lime water turns – (A) Milky on passage of carbon dioxide (C) Methyl orange red

(B) Red litmus blue (D) Yellow on passing CO2

Q.4

A student is preparing sulphur dioxide gas by reacting copper turnings and sulphuric acid. To find whether the gas is formed, he can bring the – (A) burning match stick near the mouth of jar (B) moist red litmus paper near the mouth of jar (C) moist blue litmus paper near the mouth of jar (D) moist filter paper near the mouth of jar

Q.5

Aqueous solution of a salt is acidic in nature. The salt is formed from – (A) strong acid and strong base (B) strong acid and weak base (C) weak acid and strong base (D) weak acid and weak base

Q.6

While diluting concentrated sulphuric acid, we should – (A) add concentrated acid into water (B) add water into concentrated acid (C) first add some water to acid and then add more acid (D) add acid and water in alcohol

Q.7

The chemical formula of bleaching powder is – (A) Ca(OH)2 (B) Ca(OCl)2

(C) CaCl2

Baking powder is a – (A) mixture of baking soda and citric acid (C) mixture of baking soda and tartaric acid

(B) mixture of baking soda and washing soda (D) mixture of baking soda and oxalic acid

Q.8

Q.9

Q.10

(D) CaOCl2

The acid-base indicator extracted from lichen is – (A) methyl orange (B) litmus (C) phenolphthalein

(D) vanilla extract

The chemical substance that is rubbed to give relief from wasp sting is – (A) sodium hydroxide (B) hydrochloric acid (C) sulphuric acid

(D) vinegar


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Q.11

The mixture consisting of hydrochloric acid and nitric acid in the ratio 3:1 (by parts) is known as (A) aqua fortis (B) anti-freeze (C) aqua regia (D) foal’s gold

Q.12

Acid which does not give hydrogen gas on reaction with reactive metals is – (A) acetic acid (B) hydrochloric acid (C) nitric acid (D) sulphuric acid

Q.13

Common name of H2SO4 is (A) Oil of vitriol (B) Muriatic acid

Q.14

Q.15

(C) Blue vitriol

Which one of the following relationship is correct ? 1 (A) pH   (B) pH = log [H+] (C) log pH = [H+] [H ]

(D) Green vitriol

(D) pH = log

1 [H  ]

A solution which is resistant to changes of pH on dilution or addition of small amounts of an acid or a base is known as (A) buffer solution (B) true solution (C) isohydric solution (D) ideal solution


Page # 2



Topic : Periodic Classification of Elements

DPPS. NO. – 05 .


Q.2

Q.3

Q.4

In Lother Meyer's plot, the peaks were occupied by (A) alkali metals (B) alkaline earth metals (C) halogens

(D) noble gases

Elements of which group form anions most readily ? (A) Oxygen family (B) Nitrogen family (C) Halogens

(D) Alkali metals

Diagonal relationship is not shown by (A) Li and Mg (B) C and N

(D) Be and Al

(C) B and Si

Which of the following properties does not depend on periodicity ? (A) Atomic weight (B) Electron affinity (C) Ionisation energy

(D) Electronegativity

Q.5

A sudden large jump between the values of second and third ionisation energies of an element would be associated with the electronic configuration (A) 1s2, 2s2 2p6,3s1 (B) 1s2, 2s2 2p6,3s2 3p1 2 2 6 2 2 (C) 1s , 2s 2p ,3s 3p (D) 1s2, 2s2 2p6,3s2

Q.6

The first (IE1) and second (IE2) ionisation energies (KJmol–1) of a few elements are shown below : IE1 IE2 (i) 2372 5251 (ii) 520 7300 (iii) 900 1760 (iv) 1680 3380 Which of the above elements is likely to be a noble gas ? (A) (i) (B) (ii) (C) (iii) (D) (iv)

Q.7

The element with electronic configuration 1s2 2s2 2p6 3s2 is a/an (A) Metal (B) Non- metal (C) Metalloid

(D) Inert gas

Q.8

Atomic number decides chemical property of an element. It also decides which group the element belongs to. Identify which of the following elements are from the same group in the periodic table. (A) 1, 3, 11, 19, 37 (B) 8, 24, 42, 74 (C) 4, 12, 20, 58 (D) 5, 13, 27, 47

Q.9

The radii of F, F–, O and O2– are in the order : (A) O2- > O > F- > F (B) F- > O2- > F > O

Q.10

Q.11

(C) O2- > F- > O > F

(D) O2- > F- > F > O

The total number of inner transition elements is – (A) 10 (B) 14 (C) 28

(D) 30

The following that has the largest negative electron gain enthalpy is – (A) I (B) Br (C) F

(D) Cl


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Q.12

The second ionization potential of an element M is the energy required to (A) remove one mole of electrons from one mole of gaseous atoms (B) remove one mole of electrons from one mole of gaseous anions (C) remove one mole of electrons from one mole of monovalent gaseous cations of the element (D) remove 2 moles of electrons from one mole of gaseous atoms

Q.13

The order of first ionization potential is – (A) Ca > Be > Mg (C) Mg > Be > Ca

(B) Be > Mg > Ca (D) Ca > Mg > Be

Q.14

The lower electron gain enthalpy of flourine than that of chlorine is due to its – (A) smaller size (B) smaller nuclear charge (C) difference in their electronic configurations (D) its highest reactivity

Q.15

The outermost electronic configuration of the most electronegative element is – (A) ns2 np3 (B) ns2 np4 (C) ns2 np5 (D) ns2 np6

Q.16

Eka-aluminium and Eka-silicon are known as – (A) Ga & Ge (B) Al & Si

(C) Fe & S

(D) N & Mg

Q.17

The screening effect of inner electrons on the nucleus cause – (A) a decrease in the ionization energy (B) an increase in the ionization energy (C) a decrease in atomic size (D) an increase in electro negativity

Q.18

With the increase in oxidation state of atoms, their electronegativity – (A) increases (B) decreases (C) remains unaffected (D) increases for metals and decreases for non-metals

Q.19

Elements present in the same period have – (A) same number of valence electrons (B) same number of shells in their electronic configurations (C) no relation with the electronic configuration (D) same number of electrons

Q.20

The formula of the compound formed between element X belonging to group 2 and another element Y belonging to group 15, is – (A) X3Y2 (B) X2Y3 (C) XY (D) XY3.


Page # 2


CAREER POINT PRE FOUNDATION DIVISION SUMMER WORKSHOP (IJSO) Daily Practice Problem Sheet

CHEMISTRY ANSWER KEY DPP-1 : Mole concept Q.No

1

2

3

4

5

6

7

8

9

10

11

12

13

14

15

Ans.

B

A

A

C

A

C

D

C

D

B

B

B

A

B

B

DPP-2 : Structure of atom Q.No

1

2

3

4

5

6

7

8

9

10 11 12 13 14 15 16 17 18 19 20

Ans.

D

C

A

A

A

D

A

B

D

D

D

D

B

B

D

A

A

D

D

C

DPP-3 : Chemical equations Q.No

1

2

3

4

5

6

7

8

9

10 11 12 13 14 15 16 17 18 19 20

Ans.

C

A

C

C

B

B

B

C

C

C

D

C

B

D

D

A

A

D

C

B

DPP-4 : Acids, bases & salts Q.No

1

2

3

4

5

6

7

8

9

10

11

12

13

14

15

Ans.

B

B

A

C

B

A

D

C

B

D

C

C

A

D

A

DPP-5 : Periodic Classification Q.No

1

2

3

4

5

6

7

8

9

10 11 12 13 14 15 16 17 18 19 20

Ans.

A

C

B

A

D

A

A

A

A

C

D


C

B

A

C

A

A

A

B

A

Page # 1

Chemistry

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