Question Set B

CBSE 12th Chemistry Electrochemistry Important Questions And Answers Study Material - QB365

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Questions:

Multiple Choice Question

75 x 1 = 75

A compound undergoes complete tetramerization in a given organic solvent. The van't Hoff factor (i) is

(a)

4.0

(b)

0.25

(c)

0.125

(d)

2.0

1 mole of liquid A and 2 moles of liquid B make a solution having a total vapour pressure 40 torr. The vapour pressure of pure A and pure B are 45 torr and 30 torr respectively. The above solution

(a)

is an ideal solution

(b)

shows positive deviation

(c)

shows negative deviation

(d)

is a maximum boiling azeotrope.

In which of the following cases blood cells will shrink?

(a)

When placed in water containing more than 0.9% (mass/ volume) NaCl solution

(b)

When placed in water containing less than 0.9% (mass /volume) NaCl solution

(c)

When placed in water containing 0.9% (mass/volume) NaCl solution

(d)

When placed in distilled water

The freezing point of a 0.2 molal solution of a non-electrolyte in water is (K, for water=1.86 K kg mol^-1)

(a)

-0.372°C

(b)

-1.86°C

(c)

+ 0.372°C

(d)

+ 1.86°C

Which one of the following pairs will not form an ideal solution?

(a)

Benzene and toluene

(b)

n-hexane and n-heptane

(c)

Ethanol and acetone

(d)

Bromoethane and chloroethane

\(\alpha\)-D-glucose and \(\beta\)-D-glucose differ from each other with respect to the

(a)

number of -OH groups

(b)

configuration at the C-1 carbon

(c)

size of the hemiacetal ring

(d)

configuration at the C-5 carbon

Which of the following cell is used in inverter?

(a)

Fuel cell

(b)

Mercury cell

(c)

Lead storage cell

(d)

Dry cell

Isotonic solutions have the same

(a)

density

(b)

refractive index

(c)

osmotic pressure

(d)

volume

Which of the following is correct about H-bonding in DNA?

(a)

A - T, G - C

(b)

A - G, T - G

(c)

G - T, A - C

(d)

A - A, T - T

10.

Which of the following pairs represents anomers?

(a)

(b)

(c)

(d)

11.

X(s) + 2Y⁺ (aq) \(\rightleftharpoons\) X²⁺ (aq) + 2Y(s); \(\left(\mathbf{E}_{\text {cell }}^{\circ}=\mathbf{0 . 0 5 9} \mathbf{V}\right)\)
What is the value of 'K' for above reaction?

(a)

1 x 10⁸

(b)

1 x 10²

(c)

4 x 10³

(d)

3 x 10⁴

12.

What is pH of the half cell Pt |Hz(g)| H⁺ if \(\mathbf{E}_{\mathbf{H}^{+} / \mathbf{H}_{2}}^{\circ}\) = -0.0295 V

(a)

(b)

(c)

0.5

(d)

13.

Which of the following expression is correct for 'Ka' in terms of A0 and A, where 'C' is molarity.

(a)

\(\mathbf{K}_{a}=\frac{\mathbf{C} \Lambda_{m}^{\circ}}{\Lambda_{m}\left(\Lambda_{m}^{\circ}-\Lambda\right)}\)

(b)

\(\mathbf{K}_{a}=\frac{\mathbf{C} \Lambda_{m}^{2}}{\Lambda_{m}^{0}\left(\Lambda_{m}^{0}-\Lambda_{m}\right)}\)

(c)

\(\mathbf{K}_{a}=\frac{\mathbf{C} \Lambda_{m}^{2}}{\Lambda_{m}^{\circ}}\)

(d)

\(\mathbf{K}_{a}=\frac{\mathbf{C} \Lambda_{m}^{2}}{\left(\Lambda_{m}^{0}-\Lambda_{m}\right)}\)

14.

Which of the following is correct.

(a)

K_H increases with increase in temperature (KH is Henry's law constant).

(b)

Solubility of gas in liquid decreases with increases in temperature.

(c)

K_Hdecreases with increase in temperature.

(d)

Solubility of gas in liquid increases with increase in temperature.

15.

Cone. H₂ SO₄ is 98 % H2 S04 by mass has d = 1.84 g cm₃. Volume of acid required to make one litre of 0.1 M H₂SO₄ is

(a)

5.55 mL

(b)

10 mL

(c)

20 mL

(d)

30 mL

16.

Ascorbic acid is

(a)

protein

(b)

enzyme

(c)

hormone

(d)

vitamin C

17.

Which of the following polysaccharide is stored in the cell wall in plant cells?

(a)

Cellulose

(b)

Amylose

(c)

Amylopectin

(d)

Glycogen

18.

Cellulose is

(a)

monosaccharide

(b)

disaccharide

(c)

trisaccharide

(d)

polysaccharide

19.

Sugar present in milk is

(a)

sucrose

(b)

maltose

(c)

glucos

(d)

lactose

20.

One molecule of sucrose on hydrolysis gives ___________.

(a)

2 molecules of glucose

(b)

2 moleculesof glucose + 1 moleculeof fructose

(c)

1 molecule of glucose + 1 molecule of fructose

(d)

2 moleculesof fructose

21.

Which of the following structure correctly represent the structure of glucose

(a)

(b)

(c)

(d)

22.

Which metal cannot replace H₂ from hydrochloride acid?

(a)

(b)

(c)

(d)

23.

Galvanisation is

(a)

zinc plating on aluminium sheet

(b)

zinc plating on iron sheet

(c)

iron plating on zinc sheet

(d)

aluminium plating on zinc sheet

24.

What will be the weight of silver deposited, if 96.5 A of current is passed into aqueous solution of AgNO₃ for 100 s?

(a)

1.08g

(b)

10.8g

(c)

108g

(d)

1080g

25.

The electrode potential is known as standard electrode potential

(a)

when it is reduction potential (according to IUPAC)

(b)

when concentrations of all the species involved is unity

(c)

when it is oxidation potential (according to IUPAC)

(d)

Both (a) and (b)

26.

E⁰_cell of the reactions is
Zn(s) + Cu²⁺(aq) ⇾ Zn²⁺(aq) +Cu(s);
[If E⁰ _Zn2+/Zn = -0.76, E⁰_Cu2+/Cu = 0.34V]

(a)

0.34V

(b)

-0.76V

(c)

+1.10V

(d)

-1.10V

27.

At 40°C the vapour pressure of pure liquids, benzene and toluene, are 160 mmHg and 60 mmHg respectively. At the same temperature, the vapour pressure of an equimolar solution of the two liquids, assuming the ideal solution should be

(a)

140 mmHg

(b)

110 mmHg

(c)

220 mmHg

(d)

100 mmHg

28.

In the graph given below, what does the slope of the line represent?

(a)

Partial pressure of the gas in vapour phase (\(\rho\))

(b)

Mole fraction of gas in the solution (\(\chi\))

(c)

Henry's law constant (K_H)

(d)

All of the above

29.

What will be the concentration of 0.2M H₂SO₄ solution in g/L.

(a)

21.4

(b)

39.2

(c)

9.8

(d)

19.6

30.

Which of the following is the correct example of solid solution in which the solute is in gas phase?

(a)

Copper dissolved in gold

(b)

Camphor in nitrogen gas

(c)

Hydrogen in palladium

(d)

All of these

31.

Which of the following statements are correct ?

(a)

\(\alpha \)-and \(\beta \)-D-glucopyranose are anomers

(b)

-D-glucopyranose is more stable than -D-glucopyranose

(c)

galactose is a C₄-epimer of glucose

(d)

invert sugar is laevorotatory

32.

RNA and DNA are chiral molecules, their chirality is due to

(a)

D-sugar component

(b)

L-sugar component

(c)

chiral bases

(d)

chiral phosphate ester unit

33.

The presence or absence of hydroxyl group on which carbon atom of sugar differentiates RNA and DNA?

(a)

2^nd

(b)

3^rd

(c)

4^th

(d)

1^st

34.

Which of vitamins given below is water soluble?

(a)

Vitamin E

(b)

Vitamin K

(c)

Vitamin C

(d)

Vitamin D

35.

Which functional group participates in disulphide bond formation in proteins ?

(a)

Thioether

(b)

Thiol

(c)

Thioester

(d)

Thiolactone

36.

Which statement is incorrect about peptide bond ?

(a)

C-N bond length in proteins is longer than usual bond of C^_N bond

(b)

Spectroscopic analysis shows plannar structure of -CO-NH- group

(c)

C-N bond length in proteins is smaller than usual bond length of C-N bond

(d)

None of these

37.

The number of tripeptides formed by three different amino acids are

(a)

Three

(b)

Four

(c)

Five

(d)

Six

38.

Which of the following is an essential amino acid ?

(a)

Methionine

(b)

Tyrosine

(c)

Proline

(d)

Glycine

(e)

Alanine

39.

Which of the following sets of monosaccharides forms sucrose ?

(a)

\(\alpha-D-\)galactopyranose and \(\alpha-D-\) glucopyranose

(b)

\(\alpha-D-\)galactopyranose and \(\beta-D-\)fructofuranose

(c)

\(\beta-D-\)glucopyranose and \(\beta-D-\)fructofuranose

(d)

\(\alpha-D-\)glucopyranose\(\beta-D-\)fructofuranose

40.

Proteins can be classified into two types on the basis of their molecular shape, i.e.,fibrous proteins and globular proteins. Examples of globular proteins are :

(a)

Insulin

(b)

Keratin

(c)

Cellulose

(d)

Glycogen

41.

Each polypeptide in a protein has amino acids linked with each other in a specific sequence. This sequence of amino acids is said to be .......... .

(a)

primary structure of proteins

(b)

secondary structure of proteins

(c)

tertiary structure of proteins

(d)

quaternary structure of proteins

42.

Proteins are found to have two different types of secondary structures viz. \(\alpha\) -helix and \(\beta\) - pleated sheet structure. \(\alpha\) -helix structure of protein is established by :

(a)

Peptide bonds

(b)

van der waals forces

(c)

Hydrogen bonds

(d)

Dipole-dipole interactions

43.

Glycogen is a branched chain polymer of \(\alpha\)-D-glucose units nin which chain is formed by C₁ - C₄glycosidic linkage whereas branching occures by the formation of C₁-C₆ glycosidic linkage. Structure of clycogen is similar to ......... .

(a)

Amylose

(b)

Amylopectin

(c)

Cellulose

(d)

Glucose

44.

Vitamin A is

(a)

ascorbic acid

(b)

retinol

(c)

calciferol

(d)

thiamine

45.

The number of disulphide linkages present in insulin are

(a)

(b)

(c)

(d)

46.

The letter 'D' in D-glucose signifies

(a)

configuration at all chiral carbons

(b)

dextrorotatory

(c)

that it is a monosaccharide

(d)

configuration at the penultimate chiral carbon

47.

For the cell, TI | TI⁺ (0.001 M) | Cu²⁺ (0.1 M) | Cu, E_cell at 25°C is 0.83 V. This can be increased

(a)

by increasing [Cu²⁺]

(b)

by increasing [TI⁺]

(c)

by decreasing [Cu²⁺]

(d)

by decreasing [TI⁺]

48.

Which of the following statements are not correct ?

(a)

Same quantity of electricity deposits more of iron from ferric sulphate solution than from ferrous sulphate solution

(b)

Electrochemical equivalent of an element can be obtained by dividing its equivalent weight by 96,500

(c)

1 Faraday always liberates 1 mole of the substance at the electrode

(d)

A 60 watt bulb emits 60 Joules of energy per second.

49.

In the lead-acid battery during charging, the cathode reaction is

(a)

formation of PbO₂

(b)

formation of PbSO₄

(c)

reduction of Pb²⁺ to Pb

(d)

decomposition of Pb at the anode

50.

Consider the following cell reaction :
\(2Fe(s)+{ O }_{ 2 }(g)+4{ H }^{ + }(aq)\longrightarrow { 2Fe }^{ 2+ }(aq)+2{ H }_{ 2 }O(l),{ E }^{ 0 }=1.67V\)
\(At[{ Fe }^{ 2+ }]={ 10 }^{ -3 }M,P\left( { O }_{ 2 } \right) =0.1atm\) and pH = 3, the cell potential at 25°C is

(a)

1.47 V

(b)

1.77 V

(c)

1.87 V

(d)

1.57 V

51.

The standard reduction potentials for Zn²⁺ /Zn, Ni²⁺/Ni and Fe²⁺/Fe are - 0.76, - 0.23 and - 0.44 V respectively. The reaction \(X+{ Y }^{ 2+ }\longrightarrow { X }^{ 2+ }+Y\) will be spontaneous when

(a)

X = Zn, Y = Ni

(b)

X = Ni, Y = Fe

(c)

X = Ni, Y = Zn

(d)

X = Fe, Y = Zn

52.

Small quantities of solutions of compounds TX, TY and TZ are put into separate test tubes containing X, Y and Z solutions. TX does not react with any of these. TY reacts with both X and Z. TZ reacts with X. The decreasing order of oxidation of the anions X^- , Y^- , Z^- is :

(a)

Y^-, Z^- , X^-

(b)

Z^- , X^-, Y^-

(c)

Y^- , X^- , Z^-

(d)

X^- , Z^-, Y^-

53.

Given
\({ E }_{ { Cr }^{ 3+ }/{ Cr } }^{ 0 }=-0.74V,\\ { E }_{ { MnO }_{ 4 }^{ - }/{ Mn }^{ 2+ } }^{ 0 }=1.51V\)
\({ E }_{ { CrO }_{ 7 }^{ - }/{ Cr }^{ 3+ } }^{ 0 }=1.33V,{ E }_{ Cl/{ Cl }^{ - } }^{ 0 }=1.36V\)
Based on the data given above, strongest oxidizing agent will be

(a)

MnO₄^-

(b)

Cl^-

(c)

Cr³⁺

(d)

Mn²⁺

54.

The reaction taking place in the cell
Pt | H₂ (g) | HCl (1.0 M) | AgCl | Ag is 1 atm

(a)

\(AgCl+\left( 1/2 \right) { H }_{ 2 }\longrightarrow Ag+{ H }^{ + }+{ Cl }^{ - }\)

(b)

\(Ag+{ H }^{ + }+{ Cl }^{ - }\longrightarrow AgCl+\left( 1/2 \right) { H }_{ 2 }\)

(c)

\(2{ Ag }^{ + }+{ H }_{ 2 }\longrightarrow 2Ag+2{ H }^{ + }\)

(d)

\(2Ag+2{ H }^{ + }\longrightarrow 2{ Ag }^{ + }+{ H }_{ 2 }\)

55.

Ionic mobility of Ag⁺ is (\({ \lambda }_{ { Ag }^{ + } }=5\times { 10 }^{ -4 }{ ohm }^{ -1 }{ cm }^{ 2 }{ eq }^{ -1 }\))

(a)

5.2 x 10^-9

(b)

2.4 x 10^-9

(c)

1.52 x 10^-9

(d)

8.25 x 10^-9

56.

When 0.1 mol MnO₄^2- is oxidized, the quantity of electricity required to completely oxidize MnO₄^2- to MnO₄^- is

(a)

96500 C

(b)

2 x 96500 C

(c)

9650 C

(d)

96.50 C

57.

Same quantity of electricity was passed through solutions of salts of elements A, B and C with atomic weights 7, 27 and 48 respectively. The masses of A, B and C deposited were 2.1 g , 2.7 g and 7.2 g respectively. The valencies of A, B and C respectively are

(a)

3, 2 and 1

(b)

1, 2 and 3

(c)

1, 3 and 2

(d)

2, 3 and 2

58.

Which of the following mixture do you expect will not show positive deviation from Raoult's law ?

(a)

Benzene - Chloroform

(b)

Benzene - Acetone

(c)

Benzene - Ethanol

(d)

Benzene - Carbon tetrachloride

59.

If P^o and P_s are the vapour pressures of the solvent and its solution respectively and N₁ and N₂ are the mole fractions of the solvent and solute respectively, then

(a)

P_S = P^oN₂

(b)

P^o - P_S = P^oN₂

(c)

P_S = P^oN₁

(d)

(P^o - P_S)/P_S = N₁/(N₁ + N₂).

60.

The vapour pressure of the solution M is

(a)

39.3 mm Hg

(b)

36.0 mm Hg

(c)

29.5 mm Hg

(d)

28.8 mm Hg

61.

If on dissolving the above amount of NaCl in 1 kg of water, the freezing point is found to be \(-{ 0.344 }^{ \circ }C\), the percentage dissociation of NaCl in the solution is

(a)

75%

(b)

80%

(c)

85%

(d)

90%

62.

At a certain Hill station, water boils at 96^oC. The amount of NaCI that should be added to one litre of water so that it boils at 100^oC will be (K_b for H₂O = 0.52 K/m)

(a)

[Co(NH₃)₆]CI₃

(b)

[Co(NH₃)₅CI]CI₂

(c)

[Co(NH₃)₄CI₂]CI

(d)

None of these

63.

\({ E }_{ cell }^{ \circleddash }=1.1V\) for Daniell cell. Which of the following expressions are correct description of state of equilibrium in this cell?

(a)

1.1 = K_c

(b)

\(\frac { 2.303RT }{ 2F } \log { { K }_{ c } } =1.1\)

(c)

\(\log { { K }_{ c } } =\frac { 2.2 }{ 0.059 } \)

(d)

\(\log { { K }_{ c } } =1.1\)

64.

The empirical formula of a non - electrolyte is CH₂O. A solution containing 3 g L^-1 of the compound exerts the same osmotic pressure as that of 0.05 M glucose solution. The molecular formula of the compound is

(a)

CH₂O

(b)

C₂H₄O₂

(c)

C₄H₈O₄

(d)

C₃H₆O₃

65.

The solubility of a gas in water at 300 K under a pressure of 100 atmospheres is \(4\times { 10 }^{ -3 }{ kg } \ L^{ -1 }.\) Therefore, the mass of the gas in kg dissolved in 250 mL of water under a pressure of 250 atmospheres at 300 K is

(a)

\(2.5\times { 10 }^{ -3 }\)

(b)

\(2.0\times { 10 }^{ -3 }\)

(c)

\(1.25\times { 10 }^{ -3 }\)

(d)

\(5.0\times { 10 }^{ -3 }\)

(e)

\(3\times { 10 }^{ -3 }\)

66.

Which one of the following statements is not true ?

(a)

Dissolution of all solid solutes in water is exothermic.

(b)

Common salt is more soluble in water than canesugar at the same temperature.

(c)

Solubility of sodium sulphate decahydrate crystals first increases upto a certain temperature and then decreases

(d)

Enthalphy of solution can be found using Clausius - Clapeyron equation

67.

A 5.5 molal aqueous solution of methyl alcohol, CH₃OH, is supplied. What is the mole fraction of methyl alcohol in the solution ?

(a)

0.190

(b)

0.086

(c)

0.050

(d)

0.100

68.

If Zn²⁺ / Zn electrode is diluted 100 times, then the change in emf is

(a)

increase of 59 mV

(b)

decrease of 59 mV

(c)

increase of 29.5 mV

(d)

decrease of 29.5 mV

69.

A gas X at 1 atm is bubbled through a solution containing a mixture of 1M Y^- and 1M Z^- ions at 25°C . If the reduction potential of Z > Y > X, then

(a)

Y will oxidize X but not Z

(b)

Y will oxidize both X and Z

(c)

Y will oxidize Z but not X

(d)

Y will reduce both X and Z

70.

Which of the following expressions correctly represents the equivalent conductance at infinite dilution of Al₂ (SO₄)₃. Given that \({ \lambda }^{ ° }_{ Al^{ 3+ } }\) and \({ \lambda }^{ ° }_{ { SO_{ 4 } }^{ 2- } }\) are the equivalent conductances at infinite dilution of the respective ions?

(a)

2\({ \lambda }^{ ° }_{ Al^{ 3+ } }\) +3\({ \lambda }^{ ° }_{ { SO_{ 4 } }^{ 2- } }\)

(b)

\({ \lambda }^{ ° }_{ Al^{ 3+ } }\) + \({ \lambda }^{ ° }_{ { SO_{ 4 } }^{ 2- } }\)

(c)

(\({ \lambda }^{ ° }_{ Al^{ 3+ } }\) + \({ \lambda }^{ ° }_{ { SO_{ 4 } }^{ 2- } }\) ) X 6

(d)

\(\frac{1}{3}\)\({ \lambda }^{ ° }_{ Al^{ 3+ } }\) + \(\frac{1}{2}\) \({ \lambda }^{ ° }_{ { SO_{ 4 } }^{ 2- } }\)

71.

Which of the following solution has highest equivalent conductance ?

(a)

0.01 M KCl

(b)

0.05 M KCl

(c)

0.02 M KCl

(d)

0.005 M KCl

72.

On the basis of the information given below mark the correct option.
Information: On adding acetone to methanol some of the hydrogen bonds between methanol molecules break.

(a)

At specific composition, methanol - acetone mixture will form minimum boiling azeotrope and will show positive deviation from Raoult's law.

(b)

At specific composition, methanol - acetone mixture forms maximum boiling azeotrope and will show positive deviation from Raoult's law

(c)

At specific composition methanol - acetone mixture will form minimum boiling azeotrope and will show negative deviation from Raoult's law

(d)

At specific composition methanol - acetone mixture will form maximum boiling azeotrope and will show negative deviation from Raoult's law

73.

We have three aqueous solutions of NaCI labelled as 'A', 'B' and 'C' with concentrations 0.1 M, 0.01 M, respectively. The value of van't Hoff factor for these solutions will be in the order .......... .

(a)

i_A< i_B< i_C

(b)

i_A> i_B>i_C

(c)

i_A= i_B= i_C

(d)

i_A< B > i_C

74.

The unit of ebullioscopic constant is __________________.

(a)

K kg mol^-1 or K (molality)^-1

(b)

mol kg K^-1 or K^-1 (molality)

(c)

kg mol^-1 K^-1 or K^-1 (molality)^-1

(d)

K mol kg^-1 or K (molality)

75.

In which mode of expression, the concentration of solution remains independent of temperature ?

(a)

Molarity

(b)

Normality

(c)

Formality

(d)

Molality

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Answers Key:

Multiple Choice Question

75 x 1 = 75

(b)
0.25

(a)
When placed in water containing more than 0.9% (mass/ volume) NaCl solution

(a)
-0.372°C

(b)
configuration at the C-1 carbon

(a)
A - T, G - C

10.

11.

(b)
1 x 10²

12.

13.

(b)
\(\mathbf{K}_{a}=\frac{\mathbf{C} \Lambda_{m}^{2}}{\Lambda_{m}^{0}\left(\Lambda_{m}^{0}-\Lambda_{m}\right)}\)

14.

(a)
K_H increases with increase in temperature (KH is Henry's law constant).

15.

(a)
5.55 mL

16.

(d)
vitamin C

17.

(a)
Cellulose

18.

(d)
polysaccharide

19.

(d)
lactose

20.

21.

22.

(b)
Cu

23.

(b)
zinc plating on iron sheet

24.

(b)
10.8g

25.

(d)
Both (a) and (b)

26.

27.

(b)
110 mmHg

28.

29.

(d)
19.6

30.

31.

(a)
\(\alpha \)-and \(\beta \)-D-glucopyranose are anomers

32.

(a)
D-sugar component

33.

(a)
2^nd

34.

35.

(b)
Thiol

36.

(a)
C-N bond length in proteins is longer than usual bond of C^_N bond

37.

(d)
Six

38.

(a)
Methionine

39.

(b)
\(\alpha-D-\)galactopyranose and \(\beta-D-\)fructofuranose

40.

(d)
Glycogen

41.

(a)
primary structure of proteins

42.

43.

(b)
Amylopectin

44.

(b)
retinol

45.

(a)
3

46.

(d)
configuration at the penultimate chiral carbon

47.

(a)
by increasing [Cu²⁺]

48.

(a)
Same quantity of electricity deposits more of iron from ferric sulphate solution than from ferrous sulphate solution

49.

50.

(d)
1.57 V

51.

(a)
X = Zn, Y = Ni

52.

(a)
Y^-, Z^- , X^-

53.

(a)
MnO₄^-

54.

(a)
\(AgCl+\left( 1/2 \right) { H }_{ 2 }\longrightarrow Ag+{ H }^{ + }+{ Cl }^{ - }\)

55.

(a)
5.2 x 10^-9

56.

57.

58.

(a)
Benzene - Chloroform

59.

(b)
P^o - P_S = P^oN₂

60.

(a)
39.3 mm Hg

61.

62.

(a)
[Co(NH₃)₆]CI₃

63.

(b)
\(\frac { 2.303RT }{ 2F } \log { { K }_{ c } } =1.1\)

64.

(b)
C₂H₄O₂

65.

(a)
\(2.5\times { 10 }^{ -3 }\)

66.

(a)
Dissolution of all solid solutes in water is exothermic.

67.

(b)
0.086

68.

(b)
decrease of 59 mV

69.

Reduction potentials in the order Z > Y > X means that Z can be reduced most easily and X least easily, i.e., their oxidizing powers are : Z > Y > X.

Thus, Y will oxidize X but not Z.

70.

(b)
\({ \lambda }^{ ° }_{ Al^{ 3+ } }\) + \({ \lambda }^{ ° }_{ { SO_{ 4 } }^{ 2- } }\)

71.

(d)
0.005 M KCl

72.

(a)
At specific composition, methanol - acetone mixture will form minimum boiling azeotrope and will show positive deviation from Raoult's law.

73.

74.

(a)
K kg mol^-1 or K (molality)^-1

75.

(d)
Molality

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