The equilibrium constant (K p ) for the decomposition of water H 2 O ( g ) → H 2 ( g ) + 1 2 O 2 ( g ) is given by Where α is the degree of dissociation and p is the pressure of the reaction mixture at equilibrium.

K p = α 3 / 2 P 1 / 2 ( 1 - α ) ( 2 + α ) 1 / 2

K p = α 3 P 3 2 ( 1 - α ) ( 2 + α ) 1 2

K p = α 3 P 1 2 ( 1 + α ) ( 2 - α ) 1 2

For the reaction, H 2 ( g ) + I 2 ( g ) ↔ 2 HI ( g ) the equilibrium constant K p changes with

The amounts of H 2 and I 2 present

The following equilibrium is established when hydrogen chloride is dissolved in acetic acid HCl + CH 3 COOH ↔ Cl - + CH 3 COOH 2 + The set that characterizes the conjugate acid base pair is

( HCl , Cl - ) and ( CH 3 COOH 2 + , CH 3 COOH )

( HCl , CH 3 COOH ) and ( CH 3 COOH 2 + , Cl - )

( HCl , CH 3 COOH 2 + ) and ( HCl , CH 3 COOH 2 + ) and ( CH 3 COOH , Cl - )

( CH 3 COOH 2 + , HCl ) and ( Cl - , CH 3 COOH )

The oxidation of SO 2 by O 2 to SO 3 is an exothermic reaction. The yield of SO 3 will be maximum if

Temperature is reduced and pressure is increased.

Temperature is increased and pressure is kept constant.

Both temperature and pressure are reduced.

Both temperature and pressure are increased.

Chemistry - Equilibrium - Quiz-8

At 550 K, the K_c for the following reaction is $10^{4} {mol}^{- 1} L .$

$X (g) + Y (g) ⇌ Z (g)$

At equilibrium, it was observed that

$[X] = \frac{1}{2} [Y] = \frac{1}{2} [Z]$

What is the value of [Z] at equilibrium?

0%

$10^{- 4} mol L^{- 1}$
0%

$2 \times 10^{- 4} mol L^{- 1}$
0%

$2 \times 10^{4} mol L^{- 1}$
0%

$10^{4} mol L^{- 1}$

An exothermic reaction is represented by the graph:

0%

1
0%

2.
0%

3.
0%

4.

For the reversible system ${PCl}_{3} + {Cl}_{2} ⇌ {PCl}_{5},$ the relationship between degree of dissociation $(α)$ of PCl₅ and the equilibrium constant K_p of the above equilibrium is

0%

$\frac{K_{p}}{\sqrt{P + K_{p}}}$
0%

$\sqrt{\frac{K_{p}}{1 + P . K_{p}}}$
0%

$\frac{1}{\sqrt{P + K_{p}}}$
0%

$\sqrt{\frac{1}{1 + P . K_{p}}}$

One mole of N₂O₄(g) at 300 K is kept in a closed container under one atmospheric pressure. It is heated to 600 K when 20% by mass of N₂O₄(g) decomposes to NO₂(g). The resultant pressure is

0%

1.0 atm
0%

2.4 atm
0%

2.0 atm
0%

1.2 atm

The equilibrium constant (K) of the reaction, $A + B ⇌ C + D$ at 298 K is 100. If the rate constant of the forward reaction is $4 \times 10^{5}$ , the rate constant of the reverse reaction is

0%

4
0%

$4 \times 10^{2}$
0%

$4 \times 10^{3}$
0%

$4 \times 10^{5}$

One mole of N₂O₄(g) at 310 K is 25% dissociated at 1 atm pressure. The percentage dissociation at 0.1 atm and 310 K is

0%

25%
0%

50%
0%

76%
0%

63%

K_p has the value of 10^-6 atm³ and 10^-4 atm³ at 298 K and 323 K respectively for the reaction

${CuSO}_{4} . 3 H_{2} O (s) ⇌ {CuSO}_{4} (s) + 3 H_{2} O (g) ∆_{r} H ° for the reaction is :$

0%

7.7 kJ/mol
0%

-147.41 kJ/mol
0%

147.41 kJ/mol
0%

None of these

Assume that the decomposition of HNO₃ can be represented by the following equation

$4 {HNO}_{3} (g) ⇌ 4 {NO}_{2} (g) + 2 H_{2} O (g) + O_{2} (g)$

and the reaction approaches equilibrium at 400K temperature and 30 atm pressure. At equilibrium, partial pressure of HNO₃ is 2 atm. Calculate K_c in (mol/L)³ at 400 K:

(Use : R=0.08 atm-L/mol-K)

0%

4
0%

8
0%

16
0%

32

A buffer solution can be prepared from a mixture of

I. Sodium acetate and acetic acid in water

II. Sodium acetate and hydrochloric acid in water

III. Ammonia and ammonium chloride in water

IV. Ammonia and sodium hydroxide in water.

0%

I, III, IV
0%

III, IV
0%

I, II, IV
0%

I, III

The equilibrium constant for the reactions

$N_{2} + 3 H_{2} ⇌ 2 {NH}_{3} and \frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ {NH}_{3}$

are K₁ and K₂ respectively. The correct relationship between K₁ and K₂ is

0%

$K_{1} = \frac{K_{2}}{2}$
0%

$K_{2} = \sqrt{K_{1}}$
0%

$K_{2} = {K_{1}}^{2}$
0%

$K_{1} = K_{2}$

One mole of N₂(g) is mixed with 2 moles of H₂(g) in a 4 litre vessel. If 50% of N₂(g) is converted to NH₂(g) by the following reaction:

$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g)$

What will be the value of K_c for the following equilibrium?

${NH}_{3} (g) ⇌ \frac{1}{2} N_{2} (g) + \frac{3}{2} H_{2} (g)$

0%

256
0%

16
0%

$\frac{1}{16}$
0%

None of these

If $pKa = - \log K_{a} = 4 and K_{a} = {Cx}^{2}$ then Van't Hoff factor of weak monobasic acid when C=0.01 M is

0%

1.20
0%

1.10
0%

1.02
0%

1.01

The equilibrium constant (K_p) for the decomposition of water

$H_{2} O (g) \to H_{2} (g) + \frac{1}{2} O_{2} (g)$

is given by

Where $α$ is the degree of dissociation and p is the pressure of the reaction mixture at equilibrium.

0%

$K_{p} = \frac{α^{3} P^{\frac{1}{2}}}{\sqrt{2}}$
0%

$K_{p} = \frac{α^{3} P^{\frac{3}{2}}}{(1 - α) {(2 + α)}^{\frac{1}{2}}}$
0%

$K_{p} = \frac{α^{3} P^{\frac{1}{2}}}{(1 + α) {(2 - α)}^{\frac{1}{2}}}$
0%

$K_{p} = \frac{α^{3 / 2} P^{1 / 2}}{(1 - α) {(2 + α)}^{1 / 2}}$

Which of these can not be a Bronsted acid?

0%

${HCO}_{3}^{-}$
0%

${HCOO}^{-}$
0%

$H_{2} {PO}_{3}^{-}$
0%

$H_{3} O^{+}$

In ${HS}^{-}, I^{-}, {RNH}_{2} and {NH}_{3}$ order of proton accepting tendency will be

0%

$I^{-} > {NH}_{3} > {RNH}_{2} > {HS}^{-}$
0%

${HS}^{-} > {RNH}_{2} > {NH}_{3} > I^{-}$
0%

${RNH}_{2} > {NH}_{3} > {HS}^{-} > I^{-}$
0%

${NH}_{3} > {RNH}_{2} > {HS}^{-} > I^{-}$

Which one of the following orders of acid strength is correct?

0%

$RCOOH > HC \equiv CH > HOH > ROH$
0%

$RCOOH > ROH > HOH > HC \equiv CH$
0%

$RCOOH > HOH > ROH > HC \equiv CH$
0%

$RCOOH > HOH > HC \equiv CH > ROH$

A centinormal solution of a monobasic acid is 100% ionized. Its pH is

0%

2
0%

4
0%

3
0%

1

Which of the following mixtures can act like a buffer?

0%

${CH}_{3} COOH + {CH}_{3} COONa$
0%

${NH}_{4} {NO}_{3} + {NH}_{4} OH$
0%

$50 ml 0.1 m NaCN + 30 ml 0.1 m HCl$
0%

All of the above

Which one of the following statements is not correct?

0%

Cl - is a Lewis acid
0%

the pH of $10^{- 8} M HCl$ solution is less than 7.
0%

the ionic product of water at $25 ° C$ is $10^{- 14} {mol}^{2} L^{- 2}$
0%

Bronsted-Lowry theory could not explain the acidic character of ${AlCl}_{3} .$

At $90 ° C$ , pure water has $[H_{3} O^{+}] 10^{- 6} mole {litre}^{- 1} .$ What is the value of $K_{w}$ at $90 ° C$ ?

0%

$10^{- 8}$
0%

$10^{- 6}$
0%

$10^{- 12}$
0%

$10^{- 14}$

Of the given anions, the strongest bronsted base is

0%

${ClO}_{4}^{-}$
0%

${ClO}_{3}^{-}$
0%

${ClO}_{2}^{-}$
0%

${ClO}^{-}$

The pH of a $10^{- 8}$ molar solution of HCl in water is

0%

-8
0%

8
0%

between 6 and 7
0%

between 7 and 8

An acid buffer solution can be prepared by mixing the solutions of:

0%

Sodium chloride and sodium hydroxide
0%

Sulphuric acid and sodium sulphate
0%

Ammonium chloride and ammonium nitrate
0%

Ammonium acetate and acetic acid

For the reaction, $H_{2} (g) + I_{2} (g) \leftrightarrow 2 HI (g)$ the equilibrium constant K_p changes with

0%

Catalyst
0%

Temperature
0%

Total pressure
0%

The amounts of H₂ and I₂ present

The best indicator for detection of end point in titration of a weak acid and strong base is

0%

methyl red (5 to 6)
0%

methyl orange (3 to 4)
0%

phenolphthalein (8 to 9.6)
0%

bromothymol blue (6 to 7.5)

The compound that is not a Lewis acid is-

0%

CCl₄
0%

BeCl₂
0%

BF₃
0%

AlCl₃

The conjugate acid of ${NH}_{2}^{-}$ is

0%

${NH}_{4}^{+}$
0%

${NH}_{3}$
0%

${NH}_{2} OH$
0%

$N_{2} H_{4}$

The pH of the neutralization point of 0.1 N ammonium hydroxide with 0.1 N HCl is

0%

1
0%

6
0%

9
0%

7

The compound whose 0.1 M solution is basic is

0%

Ammonium acetate
0%

Ammonium sulphate
0%

Sodium acetate
0%

Ammonium chloride

Fear or excitement, generally causes one to breathe rapidly and it results in the decrease of CO₂ concentration in blood. In what way will it change the pH of blood?

0%

pH will increase
0%

pH will decrease
0%

no change
0%

pH will adjust to 7

Which of the following is the basic buffer solution?

0%

${NH}_{4} Cl + {NH}_{4} OH$
0%

$NaCl + NaOH$
0%

${NH}_{4} Cl + {CH}_{3} COOH$
0%

${CH}_{3} COONa + {CH}_{3} COOH$

Which of the following are Lewis acids?

(i) ${BF}_{3}$

(ii) $H_{2} O$

(iii) ${HSO}_{4}^{-}$

(iv) ${SO}_{3}$

0%

(i) and (iii)
0%

(i) and (ii)
0%

(i) and (iv)
0%

(iii) and (iv)

Out of ${Ca}^{2 +}, {Al}^{3 +}, {Cr}^{3 +}, {Mg}^{2 +}, and {Zn}^{2 +},$ the reagents ${NH}_{4} Cl$ and aqueous ${NH}_{3}$ will precipitate

0%

${Ca}^{2 +}, {Al}^{3 +}$
0%

${Al}^{3 +}, {Cr}^{3 +}$
0%

${Bi}^{3 +}, {Mg}^{2 +}$
0%

${Mg}^{2 +}, {Zn}^{2 +}$

Which among the following is the least soluble?

0%

$MnS (K_{sp} = 7 \times 10^{- 16})$
0%

$FeS (K_{sp} = 4 \times 10^{- 19})$
0%

$PtS (K_{sp} = 8 \times 10^{- 73})$
0%

$NiS (K_{sp} = 3 \times 10^{- 12})$

The dissociation constant of a substituted benzoic acid at $25 ° C$ is $1 \times 10^{- 4} .$ The pH of a 0.01 m solution of its sodium salt of benzoic acid is

0%

6
0%

7
0%

8
0%

9

Which one of the following is true for any diprotic acid, $H_{2} X$ ?

0%

${Ka}_{1} = {Ka}_{2}$
0%

${Ka}_{2} > {Ka}_{1}$
0%

${Ka}_{1} > {Ka}_{2}$
0%

${Ka}_{2} = 1 / {Ka}_{1}$

For sparingly soulble salt $A_{p} B_{q}$ , the relationship of its solubility product $(L_{s})$ with its solubility (s) is

0%

$L_{s} = s^{p + q} . p^{p} . q^{q}$
0%

$L_{s} = s^{p + q} . p^{q} . q^{q}$
0%

$L_{s} = s^{pq} p^{q} q^{q}$
0%

$L_{s} = s^{pq} . {(pq)}^{p + q}$

pKa values of three acids A, B and C are 4.3, 3.3 and 5.5 respectively. Which of the following represents the correct order of acid strength?

0%

A>B>C
0%

C>A>B
0%

B>A>C
0%

C>B>A

Which of the following statements is correct?

I. The pH of $1.0 \times 10^{- 8} M$ solution of HCl is 8

II. The conjugate base of $H_{2} {PO}_{4}^{-}$ is ${HPO}_{4}^{2 -}$

III. Autoprotolysis constant of water increases with temperature

IV. When a solution of a weak monoprotic acid is titrated against a strong base at half neutralization point, pH = (1/2) pKa.

0%

II, III
0%

I, II, III
0%

III, IV
0%

II, III, IV

The solubility of $A_{2} X_{3}$ is y mol dm^-3. Its solubility product is

0%

$6 y^{4}$
0%

$64 y^{4}$
0%

$36 y^{5}$
0%

$108 y^{5}$

If ${pK}_{b}$ for fluoride ion at $25 ° C$ is 10.83, the ionization constant of hydrofluoric acid at this temperature is

0%

$1.74 \times 10^{- 5}$
0%

$3.52 \times 10^{- 3}$
0%

$6.75 \times 10^{- 4}$
0%

$5.38 \times 10^{- 2}$

The pK_a of HCN is 9.30. The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles of HCN in water and making up the total volume to 500 ml will be:

0%

9.30
0%

8.30
0%

7.30
0%

10.30

What is the decreasing order of strength of the bases?

${OH}^{-}, {NH}_{2}^{-}, H - C \equiv C^{-} and {CH}_{3} - {CH}_{2}^{-} ?$

0%

${CH}_{3} - {CH}_{2}^{-} > {NH}_{2}^{-} > H - C \equiv C^{-} > {OH}^{-}$
0%

$H - C \equiv C^{-} > {CH}_{3} - {CH}_{2}^{-} > {NH}_{2}^{-} > {OH}^{-}$
0%

${OH}^{-} > {NH}_{2}^{-} > H - C \equiv C^{-} > {CH}_{3} - {CH}_{2}^{-}$
0%

${NH}_{2}^{-} > H - C \equiv C^{-} > {OH}^{-} > {CH}_{3} - {CH}_{2}^{-}$

The following equilibrium is established when hydrogen chloride is dissolved in acetic acid

$HCl + {CH}_{3} COOH \leftrightarrow {Cl}^{-} + {CH}_{3} {COOH}_{2}^{+}$

The set that characterizes the conjugate acid base pair is

0%

$(HCl, {CH}_{3} COOH) and ({CH}_{3} {COOH}_{2}^{+}, {Cl}^{-})$
0%

$(HCl, {CH}_{3} {COOH}_{2}^{+}) and (HCl, {CH}_{3} {COOH}_{2}^{+}) and ({CH}_{3} COOH, {Cl}^{-})$
0%

$({CH}_{3} {COOH}_{2}^{+}, HCl) and ({Cl}^{-}, {CH}_{3} COOH)$
0%

$(HCl, {Cl}^{-}) and ({CH}_{3} {COOH}_{2}^{+}, {CH}_{3} COOH)$

Which of the following is an example of a reversible reaction?

0%
${KNO}_{3} (aq) + NaCl (aq) ⇌ KCl (aq) + {NaNO}_{3} (aq)$
0%
$2 Na (s) + H_{2} O (l) ⇌ 2 NaOH (aq) + H_{2} (g)$
0%
${AgNO}_{3} (aq) + HCl (aq) ⇌ AgCl (s) + {NaNO}_{3} (aq)$
0%
$Pb {({NO}_{3})}_{2}_{(aq)} + 2 {NaI}_{(aq)} ⇌ {PbI}_{2}_{(s)} + {NaNO}_{3 (aq)}$

A certain weak acid has a dissociation constant of $1.0 \times 10^{- 4} .$ The equilibrium constant for its reaction with a strong base is

0%

$1.0 \times 10^{10}$
0%

$1.0 \times 10^{14}$
0%

$1.0 \times 10^{- 10}$
0%

$1.0 \times 10^{- 4}$

The precipitate of CaF₂ $(K_{sp} = 1.7 \times 10^{- 10})$ is obtained when equal volumes of the following are mixed

0%

$10^{- 2} M {Ca}^{2 +} + 10^{- 3} {MF}^{-}$
0%

$10^{- 3} M {Ca}^{2 +} + 10^{- 5} {MF}^{-}$
0%

$10^{- 4} M {Ca}^{2 +} + 10^{- 4} {MF}^{-}$
0%

$10^{- 5} M {Ca}^{2 +} + 10^{- 3} {MF}^{-}$

The oxidation of SO₂ by O₂ to SO₃ is an exothermic reaction. The yield of SO₃ will be maximum if

0%

Temperature is reduced and pressure is increased.
0%

Temperature is increased and pressure is kept constant.
0%

Both temperature and pressure are reduced.
0%

Both temperature and pressure are increased.

If a solution of 0.1 M NH4OH and 0.1 M NH₄Cl has pH 9.25, then the pK_b of NH₄OH will be:

0%

9.25
0%

4.75
0%

3.75
0%

8.25

The solubility of MX₂ type electrolyte is $0.5 \times 10^{- 4}$ mol L^-1. Then find out K_sp of electrolytes.

0%

$5 \times 10^{- 12}$
0%

$25 \times 10^{- 10}$
0%

$1 \times 10^{- 13}$
0%

$5 \times 10^{- 13}$

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Practice Chemistry Quiz Questions and Answers

0:0:1

Practice Chemistry Quiz Questions and Answers

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