In the reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g ) , when 100 mL of N 2 has reacted, the volumes of H 2 and NH 3 are

300 mL of H 2 and 200 mL of NH 3

300 mL of H 2 and 300 mL of NH 3

100 mL of H 2 and 200 mL of NH 3

100 mL of H 2 and 100 mL of NH 3

The reaction PCl 5 ( s ) ⇌ PCl 3 ( g ) + Cl 2 ( g ) is in equilibrium. If the equilibrium concentration of PCl 3 (g) is doubled, then the concentration of Cl 2 (g) would become

four times of its initial value

Two moles of N 2 O 4 is heated to form NO and O 2 . As soon as NO and O 2 are formed they react to form N 2 O 5 . Two equilibria N 2 O 4 ⇌ 2 NO + O 2 2 NO + 3 2 O 2 ⇌ N 2 O 5 Are simultaneously established. At equilibrium, the degree of dissociation of N 2 O 4 was found to 50%. Which of the following is correct at equilibrium?

1 2 [ N 2 O 5 ] + [ O 2 ] = 1 2 [ NO ]

2 [ N 2 O 4 ] = [ NO ] + 3 2 [ O 2 ] + [ N 2 O 5 ]

[ NO ] + [ O 2 ] = [ N 2 O 4 ] + [ N 2 O 5 ]

For the reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g ) at 500 ° C , the value of K p is 1 . 44 × 10 - 5 when the partial pressure are measured in atmosphere. The value of K c with concentration in mol L -1 is

1 . 44 × 10 - 5 ( 0 . 082 × 773 ) - 2

1 . 44 × 10 - 5 ( 8 . 314 × 773 ) - 2

1 . 44 × 10 - 5 ( 0 . 082 × 500 ) - 2

1 . 44 × 10 - 5 ( 0 . 081 × 773 ) - 2

Chemistry - Equilibrium - Quiz-7

$\underset{g}{{PCl}_{5}} ⇌ \underset{g}{{PCl}_{3}} + \underset{g}{{Cl}_{2}}$

For the dissociation of PCl_5- K_c is $2 \times 10^{- 7} at 27 ° C$ .

$Find ∆ S ° If ∆ H ° = 28.4 KJ / m$

0%

-0.0336 KJ/K
0%

0.0336 KJ/K
0%

-0.0818 KJ/K
0%

0.338 KJ/K

The value of K_p for the reaction,

$2 H_{2} S (g) ⇌ 2 H_{2} (g) + S_{2} (g) is 1.2 \times 10^{- 2} at 1065 ° C .$

The value of K_c is

0%

$< 1.2 \times 10^{- 2}$
0%

$> 1.2 \times 10^{- 2}$
0%

$1.2 \times 10^{- 2}$
0%

$0.12 \times 10^{- 2}$

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to the concentrations of the conjugate acid (HIn) and base (In^-) forms of the indicator by the expression:

0%

$\log [\frac{{In}^{-}}{HIn}] = {pK}_{In} - pH$
0%

$\log [\frac{HIn}{{In}^{-}}] = {pK}_{In} + pH$
0%

$\log [\frac{HIn}{In}] = pH - {pK}_{In}$
0%

$\log [\frac{In}{HIn}] = pH - {pK}_{In}$

In the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g),$ when 100 mL of N₂ has reacted, the volumes of H₂ and NH₃ are

0%

300 mL of H₂ and 300 mL of NH₃
0%

100 mL of H₂ and 200 mL of NH₃
0%

300 mL of H₂ and 200 mL of NH₃
0%

100 mL of H₂ and 100 mL of NH₃

If a mixture containing 3 moles of hydrogen and 1 mole of nitrogen is converted completely into ammonia, the ratio of volumes of reactants and products at the same temperature and pressure would be

0%

2:1
0%

1:2
0%

1:3
0%

3:1

Equilibrium constant for the reaction

$2 A (g) ⇌ B (g) + C (g)$ at 780 k and 10 atm pressure is 3.52. The equilibrium constant of this reaction at 780 k and 20 atm pressure is

0%

5.72
0%

11.44
0%

28.6
0%

3.52

For the reaction, $A + B ⇌ C + D$ , the rate constants for the forward and backward reactions are found to be $4.2 \times 10^{- 2}$ and $3.36 \times 10^{- 3} mol L^{- 1} s^{- 1}$ respectively. What is the equilibrium constant for the reaction?

0%

11.5
0%

12.5
0%

8.0
0%

6.0

In the reaction $2 H_{2} S (g) ⇌ 2 H_{2} (g) + S_{2} (g)$ the concentration of H₂S is 0.5 mol L^-1 and concentration of H₂ is 0.1 mol L^-1 while concentration of S₂ is 0.4 mol L^-1 in one litre vessel. The value of equilibrium constant of the reaction is

0%

0.016
0%

0.013
0%

0.020
0%

0.030

For a gaseous reaction , $2 A + B ⇌ C + D,$

the partial pressure of A, B, C and D at equilibrium are 0.5, 0.8, 0.7 and 1.2 atm. The value of K_p for this reaction is

0%

2.4 atm
0%

6.2 atm^-2
0%

4.2 atm^-1
0%

8.4 atm^-3

For the reaction $C (s) + {CO}_{2} (g) ⇌ 2 CO (g),$ the partial pressure of CO₂ and CO are 4 and 8 atm respectively. The value of K_p for this reaction is

0%

14 atm
0%

16 atm
0%

18 atm
0%

12 atm

In which of the following gaseous reaction, K_p and K_c have the same values?

0%

$2 HI ⇌ H_{2} + I_{2}$
0%

$N_{2} + 3 H_{2} ⇌ 2 {NH}_{3}$
0%

$2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3}$
0%

${PCI}_{5} ⇌ {PCII}_{3} + {Cl}_{2}$

In which of the following gaseous reaction, the value of K_p is less than K_c?

0%

${PCl}_{5} ⇌ {PCl}_{3} + {Cl}_{2}$
0%

$N_{2} + O_{2} ⇌ 2 NO$
0%

$2 HI ⇌ H_{2} + I_{2}$
0%

$N_{2} + 3 H_{2} ⇌ {NH}_{3}$

The value of K_c for the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g)$ at 400 is 0.5. The value of K_p for the reactions is $(R = 0.0821 L atm {mol}^{- 1} K^{- 1})$

0%

$25.6 \times 10^{- 2}$
0%

$4.6 \times 10^{- 4}$
0%

$46.6 \times 10^{- 4}$
0%

$16.6 \times 10^{- 8}$

The value of K_p for the reaction,

$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g) at 700 is 1.3 \times 10^{- 3} {atm}^{- 1} .$ The value of K_c at same temperature will be

0%

$1.4 \times 10^{- 2}$
0%

$7.4 \times 10^{- 2}$
0%

$5.2 \times 10^{- 2}$
0%

$3.1 \times 10^{- 2}$

The ratio of $\frac{K_{p}}{K_{c}}$ for the reaction

${SO}_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {SO}_{3} (g) is$

0%

(RT)^-1/2
0%

(RT)^1/2
0%

(RT)
0%

1

$If 2 \underset{g}{NO} ⇌ N_{2} + O_{2} K_{c_{1}} = 2.5 \times 10^{30} \underset{g}{NO} + \frac{1}{2} \underset{g}{{Br}_{2}} ⇌ \underset{g}{NOBr} K_{c_{2}} = 1.6$

find K_c for the reaction given below

$\frac{1}{2} \underset{g}{N_{2}} + \frac{1}{2} \underset{g}{O_{2}} + \frac{1}{2} \underset{g}{{Br}_{2}} ⇌ \underset{g}{NOBr}$

0%

$1.01 \times 10^{- 15}$
0%

$2.02 \times 10^{- 15}$
0%

$1.01 \times 10^{30}$
0%

$2.02 \times 10^{15}$

If K_p of the reaction $A (g) + 2 B (g) ⇌ 3 C (g) + D (g)$ is 0.05 at 1000 K, then the value of K_c of the reaction

0%

20000 R
0%

0.02 R
0%

$\frac{5 \times 10^{- 5}}{R}$
0%

$5 \times 10^{- 5} R$

The reaction ${PCl}_{5} (s) ⇌ {PCl}_{3} (g) + {Cl}_{2} (g)$ is in equilibrium. If the equilibrium concentration of PCl₃(g) is doubled, then the concentration of Cl₂(g) would become

0%

1/2 of its initial value
0%

1/4 of its initial value
0%

four times of its initial value
0%

two times of its initial value

In the reaction, the equilibrium concentrations of PCl₅ and PCl₃ are 0.4 and 0.2 mole/liter respectively. If the value of K_c is 0.5, what is the concentration of Cl₂ in mole/liter?

0%

2.0
0%

1.5
0%

1.0
0%

0.5

4 moles each of SO₂ and O₂ gases are allowed to react to form SO₃ in a closed vessel. At equilibrium, 25% of O₂ is used up. The total number of moles of all the gases at equilibrium is

0%

6.5
0%

7.0
0%

8.0
0%

2.0

For the reversible reaction,

N2(g)+3H2(g)⇌2NH3(g)

At 500°C, the value of K_p is 1.44×10^-5 when partial pressure is measured in atmospheres. The corresponding value of K_c, with concentration in mole L^-1, is

0%

1.44×10^-5(0.082×500)^-2
0%

1.44×10^-5/(8.314×773)^-2
0%

1.44×10^-5(0.082×773)^-2
0%

1.44×10^-5/(0.082×773)^-2

If N₂O₄ is dissociation to 33% and 40% at total pressure P₁ and P₂ atm respectively. The ratio of $\frac{P_{1}}{P_{2}}$ is

0%

$\frac{8}{5}$
0%

$\frac{5}{8}$
0%

$\frac{9}{5}$
0%

$\frac{5}{9}$

For which of the following reaction, $K_{p} = K_{c} ?$

0%

$2 NOCl (g) ⇌ 2 NO (g) + {Cl}_{2} (g)$
0%

$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g)$
0%

$H_{2} (g) + {Cl}_{2} (g) ⇌ 2 HCl (g)$
0%

${PCl}_{3} (g) + {Cl}_{2} (g) ⇌ {PCl}_{5} (g)$

In which of the following reactions, equilibrium is independent of pressure?

0%

$N_{2} (g) + O_{2} (g) ⇌ 2 NO (g); ∆ H = + ve$
0%

$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g); ∆ H = - ve$
0%

$3 H_{2} (g) + N_{2} (g) ⇌ 2 {NH}_{3} (g); ∆ H = - ve$
0%

${PCl}_{5} (g) ⇌ {PCl}_{3} (g) + {Cl}_{2} (g); ∆ H = + ve$

The equilibrium constant of mutarotation of $α$ -D-glucose to $β$ -D-glucose is 1.8. What percent of the $α$ -form remains under equilibrium?

0%

35.7
0%

64.3
0%

55.6
0%

44.4

For a gaseous equilibrium

$2 A (g) ⇌ 2 B (g) + C (g),$ K_p has a value of 1.8 at 700 K. What is the value of K_c for the equilibrium $2 B (g) + C (g) ⇌ 2 A$ (g) at the same pressure?

0%

0.031
0%

$1.3 \times 10^{- 3}$
0%

44.4
0%

38

Two moles of N₂O₄ is heated to form NO and O₂. As soon as NO and O₂ are formed they react to form N₂O₅. Two equilibria

$N_{2} O_{4} ⇌ 2 NO + O_{2} 2 NO + \frac{3}{2} O_{2} ⇌ N_{2} O_{5}$

Are simultaneously established. At equilibrium, the degree of dissociation of N₂O₄ was found to 50%. Which of the following is correct at equilibrium?

0%

$\frac{1}{2} [NO] = \frac{3}{2} [O_{2}]$
0%

$2 [N_{2} O_{4}] = [NO] + \frac{3}{2} [O_{2}] + [N_{2} O_{5}]$
0%

$[NO] + [O_{2}] = [N_{2} O_{4}] + [N_{2} O_{5}]$
0%

$\frac{1}{2} [N_{2} O_{5}] + [O_{2}] = \frac{1}{2} [NO]$

Solubility of a M₂S salt is $3.5 \times 10^{- 6}$ then find out solubility product.

0%

$1.7 \times 10^{- 6}$
0%

$1.7 \times 10^{- 16}$
0%

$1.7 \times 10^{- 18}$
0%

$1.7 \times 10^{- 12}$

The equilibrium constants for the given reactions are:

$H_{3} {PO}_{4} ⇌ H^{+} + H_{2} {PO}_{4}^{-} is K_{1}, H_{2} {PO}_{4} ⇌ H^{+} + {HPO}_{4}^{2 -} is K_{2} and {HPO}_{4}^{2 -} ⇌ H^{+} + {PO}_{4}^{3 -} is K_{3} .$

The equilibrium constant (K) for

$H_{3} {PO}_{4} ⇌ 3 H^{+} + {PO}_{4}^{3 -} will be$

0%

$K_{1} \times K_{2} \times K_{3}$
0%

$K_{1} / K_{2} K_{3}$
0%

$K_{2} / K_{1} K_{3}$
0%

$K_{1} + K_{2} + K_{3}$

The equilibrium constants for the reactions,

${XeF}_{6} (g) + H_{2} O (g) ⇌ {XeOF}_{4} (g) + 2 HF (g) . . . . . . . . (i)$

$and {XeO}_{4} (s) + {XeF}_{6} (g) ⇌ {XeOF}_{4} (g) + {XeO}_{3} F_{2} (g) . . . . . . (ii)$

are K₁ and K₂ respectively. The equilibrium constant (K) for the reaction

${XeO}_{4} (g) + 2 HF (g) ⇌ {XeO}_{3} F_{2} (g) + H_{2} O (g) is$

0%

$K_{1} / K_{2}$
0%

$K_{2} / K_{1}$
0%

K₁=2K₂
0%

K₂=1K₁

In a 0.5 litre capacity vessel, CO and Cl₂ are mixed to form COCl₂. At equilibrium, it contains 0.2 mole of COCl₂ and 0.1 mole each of CO and Cl₂. The equilibrium constant (K_c) for reaction

$CO + {Cl}_{2} ⇌ {COCl}_{2} is$

0%

15
0%

5
0%

20
0%

10

An equilibrium mixture for the reaction,

$2 H_{2} S (g) ⇌ 2 H_{2} (g) + S_{2} (g)$

had 1 mole of H₂S, 0.2 mole of H₂ and 0.8 mole of S₂ in a 2 litre flask. The value of K_c in mol L^-1 is

0%

0.08
0%

0.016
0%

0.004
0%

0.160

1.25 moles of NOCl were placed in a 2.50 L reaction chamber at $427 ° C .$ After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant K_c for the reaction,

$2 NOCl (g) ⇌ 2 NO (g) + {Cl}_{2} (g)$

0%

$1.6 \times 10^{- 3}$
0%

$5.6 \times 10^{- 4}$
0%

$2.6 \times 10^{- 3}$
0%

$4.6 \times 10^{- 4}$

If equilibrium constant for the reaction,

${XO}^{-} (q) + H_{2} O (l) ⇌ HXO (aq) + {OH}^{-} (aq)$

is $0.3 \times 10^{- 6}$ then find the value of dissociation constant (K_a) for HXO?

0%

$0.36 \times 10^{- 8}$
0%

$2.8 \times 10^{- 8}$
0%

$2.8 \times 10^{- 10}$
0%

$0.36 \times 10^{- 6}$

The equilibrium constant value for the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g) is 1.48 \times 10^{- 5}$ , the value for the reaction $1 / 2 N_{2} (g) + 3 / 2 H_{2} (g) ⇌ {NH}_{3} (g) is n \times 10^{- 3}$ where n is

0%

1.85
0%

3.85
0%

4.85
0%

10

A gaseous phase reaction is allowed to attain equilibrium as $A (g) ⇌ B (g) + C (g)$ at constant pressure P. The partial pressure of A at equilibrium is P/2. The value of equilibrium constant K_p is

0%

$\frac{P}{8}$
0%

$\frac{P}{6}$
0%

$\frac{P}{2}$
0%

$\frac{P}{4}$

${NH}_{4} HS (s) ⇌ {NH}_{3} (g) + H_{2} S (g)$

The equilibrium pressure at $25 ° C$ is 0.660 atm. What is K_p for the reaction?

0%

0.109
0%

0.218
0%

1.89
0%

2.18

K_c for the reaction ${SO}_{2} (g) + {NO}_{2} (g) ⇌ {SO}_{3} (g) + NO (g)$ is 16 at a given temperature. If we take one mole each of all the four gases in one litre vessel, the equilibrium concentration of SO₂ and SO₃ respectively in mol L^-1 are

0%

0.4, 0.8
0%

0.8, 0.16
0%

1.6, 0.8
0%

0.4, 1.6

The ratio of ${{K_{P}}\over{K_{C}}}$ for the reaction

$CO (g) + \frac{1}{2} O_{2} (g) ⇌ {CO}_{2} (g) is$

0%

(RT)^1/2
0%

(RT)^-1/2
0%

RT
0%

1

Determine the value of equilibrium constant (K_c) for the reaction

$A_{2} (g) + B_{2} (g) ⇌ 2 AB (g)$

If 10 moles of A₂; 15 moles of B₂ and 5 moles of AB are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of AB is 7.5 M:

0%

4.5
0%

1.5
0%

0.6
0%

None of these

A 1 M solution of glucose reaches dissociation equilibrium given below.

$C_{6} H_{12} O_{6} ⇌ 6 HCHO$

If the equilibrium constant is $0.167 x 10^{- 22}$ , the concentration of HCHO in the equilibrium is

0%

$1.60 \times 10^{- 8} M$
0%

$3.20 \times 10^{- 6} M$
0%

$3.20 \times 10^{- 4} M$
0%

$1.60 \times 10^{- 4} M$

For the dissociation reaction $N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g)$ the degree of dissociation $(α)$ in terms of K_p and total equilibrium pressure P is:

0%

$α = \sqrt{\frac{4 P + K_{p}}{K_{p}}}$
0%

$α = \sqrt{\frac{K_{p}}{4 P + K_{p}}}$
0%

$α = \sqrt{\frac{K_{p}}{4 P}}$
0%

None of these

When CO₂ dissolves in water, the following equilibrium is established.

${CO}_{2} + 2 H_{2} O ⇌ H_{3} O^{+} + H {CO}_{3}^{-}$

The equilibrium constant is $3.8 \times 10^{- 7}$ and at pH=6.0, the ratio $\frac{[{HCO}_{3}^{-}]}{[{CO}_{2}]}$ will be

0%

$3.8 \times 10^{- 13}$
0%

$3.8 \times 10^{- 1}$
0%

6.0
0%

13.4

At certain temperature compound AB₂(g) dissociates according to the reaction

$2 {AB}_{2} (g) ⇌ 2 AB (g) + B_{2} (g)$

The value of K_p in terms of degree of dissociation $' α'$ and total pressure 'P' is

0%

$P \frac{α^{3}}{2}$
0%

$P \frac{α^{2}}{3}$
0%

$P \frac{α^{3}}{3}$
0%

$P \frac{α^{2}}{2}$

When NaNO3 is heated in a closed vessel, O2 is liberated and NaNO2 is left behind. At equilibrium:

0%

Addition of NaNO2 favours reverse reaction
0%

Addition of NaNO3 favours forward reaction
0%

Increasing temperature favours forward reaction.
0%

None of these

An element X being with oxygen and CO present in air as

$X (g) + O_{2} (g) ⇌ {XO}_{2} (g); K_{p_{1}} = 27 X (g) + CO (g) ⇌ XCO (g); K_{p_{2}} = 10^{4}$

When X at 1 atm is treated with air, 25% of it is bound to CO(g). The partial pressure of CO(g) in air at equilibrium, if partial pressure of O₂(g) in air at equilibrium is 0.2 atm, would be

0%

$1.9 \times 10^{4} atm$
0%

$1.9 \times 10^{- 4} atm$
0%

$2.08 \times 10^{4} atm$
0%

$2.08 \times 10^{- 4} atm$

A 250 ml flask containing NO(g) at 0.46 atm is connected to a 100 ml flask containing oxygen gas at 0.86 atm by means of a stop cock at 350 K, the gases are mixed by opening the stop cock where the following equilibrium is established.

$\underset{g}{2 NO} + O_{2} \to \underset{g}{2 {NO}_{2}} ⇌ \underset{g}{N_{2} O_{4}}$

The first reaction is complete while the second is at equilibrium. If thetotal pressure is 0.37 atm, K_p is

0%

0.645 atm^-1
0%

1.290 atm^-1
0%

20 atm^-1
0%

5.46 atm^-1

For the reaction (i) and (ii)

$A (g) ⇌ B (g) + C (g) . . . . . . . . . . . (i) X (g) ⇌ 2 Y (g) . . . . . . . . . . . . . (ii)$

Given, $K_{p_{1}} : K_{p_{2}} = 9 : 1 .$ If degree of dissociation of A(g) and X(g) are same then the ratio of total pressure in equilibrium (i) and (ii) will be

0%

36:1
0%

0.5:1
0%

1:1
0%

3:1

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g) at 500 ° C,$ the value of K_p is $1.44 \times 10^{- 5}$ when the partial pressure are measured in atmosphere. The value of K_c with concentration in mol L^-1 is

0%

$\frac{1.44 \times 10^{- 5}}{{(8.314 \times 773)}^{- 2}}$
0%

$\frac{1.44 \times 10^{- 5}}{{(0.082 \times 500)}^{- 2}}$
0%

$\frac{1.44 \times 10^{- 5}}{{(0.081 \times 773)}^{- 2}}$
0%

$\frac{1.44 \times 10^{- 5}}{{(0.082 \times 773)}^{- 2}}$

The degree of dissociation of PCl₅ at one atmosphere is 0.3. The pressure at which PCl₅ is dissociated to 50% is

0%

0.273 atm
0%

0.3 atm
0%

1.34 atm
0%

2.73 atm

0:0:1

Practice Chemistry Quiz Questions and Answers

0:0:1

Practice Chemistry Quiz Questions and Answers

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