A reaction S 8 ( g ) ⇌ 4 S 2 ( g ) is carried out by taking 2 moles of S 8 ( g ) and 0 . 2 mole of S 2 ( g ) in a reaction vessel of 1 litre at 900 K . Which are correct if K C = 6 . 30 × 10 - 6 ?

Reaction proceeds in forward direction.

If the equilibrium constant of the reaction 2 HI ( g ) ⇌ H 2 ( g ) + I 2 ( g ) is 0 . 25 , then the equilibrium constant of the reaction H 2 ( g ) + I 2 ( g ) ⇌ 2 HI ( g ) will be?

For the chemical reaction 2 HI ( g ) ⇌ H 2 ( g ) + I 2 ( g ) , K C = 0 . 25 Doing the reverse of the reaction, we get: 2 HI g ⇌ H 2 g + I 2 g . . . K c ' = 1 K c = 1 0 . 25 = 4 The equilibrium expression written for a reaction in the reverse direction is the reciprocal of the one for the forward reaction, i.e. K ' = 1 K .

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When ethanol and acetic acid were mixed together in an equimolar proportion, $66.6 %$ is converted into ethyl acetate. Calculate $K_{C}$ . Also, calculate the quantity of ester produced, if one mole of acetic acid is treated with $0.5 mol$ and $4 mol$ of alcohol, respectively.

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Important Questions on Chemical Equilibrium

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 18

In an aqueous solution of volume

500 mL

, when the reaction of

2 {Ag}^{+} + Cu ⇌ {Cu}^{2 +} + 2 Ag

has reached the equilibrium,

[{Cu}^{2 +}]

was

x M

. When

500 mL

of water is further added at equilibrium,

[{Cu}^{2 +}]

will be

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 19

Consider following reactions in equilibrium concentration

0.01 M

of every species.

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

(II) 2 {HI}_{(g)} ⇌ {H_{2}}_{(g)} + {I_{2}}_{(g)}

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

The extent of the reactions taking place is

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 20

For the reaction, $N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g)$ , the value of $K$ is $50$ at $400 K$ and $1700$ at $500 K$ . Which of the following option(s) is/are correct?

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 21

A reaction

S_{8} (g) ⇌ 4 S_{2} (g)

is carried out by taking

2 moles

S_{8} (g)

and

0.2 mole

S_{2} (g)

in a reaction vessel of

1 litre

900 K

. Which are correct if

K_{C} = 6.30 \times 10^{- 6} ?

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 22

(a) ${N_{2}}_{(g)} + {O_{2}}_{(g)} ⇌ 2 {NO}_{(g)}; K_{1}$
(b) $(\frac{1}{2}) {N_{2}}_{(g)} + (\frac{1}{2}) {O_{2}}_{(g)} ⇌ NO (g); K_{2}$
(c) $2 {NO}_{2}_{(g)} ⇌ {N_{2}}_{(g)} + {O_{2}}_{(g)}; K_{3}$
(d) ${NO}_{(g)} ⇌ (\frac{1}{2}) {N_{2}}_{(g)} + (\frac{1}{2}) {O_{2}}_{(g)}; K_{4}$

The correct relation between $K_{1}, K_{2}, K_{3}$ and $K_{4}$ is/are

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 24

If the equilibrium constant of the reaction

2 HI (g) ⇌ H_{2} (g) + I_{2} (g)

0.25

, then the equilibrium constant of the reaction

H_{2} (g) + I_{2} (g) ⇌ 2 HI (g)

will be?

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 25

For the reaction involving the oxidation of ammonia by oxygen to form nitric oxide and water vapour, the equilibrium constant has the units $(bar)^{n}$ . Then, $n$ is:

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JEE Main

IMPORTANT

Chapterwise/Topicwise Daily Practice Problems (DPP) Physical Chemistry Part 1 JEE Main & Advanced>Chapter 6 - Chemical Equilibrium>DPP 6.2>Q 26

For the equilibrium of the reaction,

{NH}_{4} {Cl}_{(s)} ⇌ {NH}_{3}_{(g)} + {HCl}_{(g)}, K_{p} = 81 {atm}^{2}

. The total pressure at equilibrium will be

x

times the pressure of

{NH}_{3}

. The value of

x

will be?

When ethanol and acetic acid were mixed together in an equimolar proportion, 66.6% is converted into ethyl acetate. Calculate KC. Also, calculate the quantity of ester produced, if one mole of acetic acid is treated with 0.5 mol and 4 mol of alcohol, respectively.

Important Questions on Chemical Equilibrium

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When ethanol and acetic acid were mixed together in an equimolar proportion, $66.6 %$ is converted into ethyl acetate. Calculate $K_{C}$ . Also, calculate the quantity of ester produced, if one mole of acetic acid is treated with $0.5 mol$ and $4 mol$ of alcohol, respectively.