Graph of a reversible process; N 2 + 3 H 2 ⇌ 2 NH 3 + Heat is given. Analyse the graph and answer the following question. Identify the part of the graph which represents the forward reaction [ OA, BA, AC]

BA part of the graph represents the forward reaction. The forward reaction speeds up temporarily as a result of the addition of reactants. The position of equilibrium shifts as more ammonia ( NH 3 ) is produced. The concentration of ammonia increases, while the concentration of N 2 and H 2 decreases. The forward reaction in the production of ammonia is exothermic.

MEDIUM

Earn 100

Explain homogeneous equilibrium with the help of an example.

Important Questions on Equilibrium

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

A homogeneous ideal gaseous reaction

{AB}_{2 (g)} ⇌ A_{(g)} + 2 B_{(g)}

is carried out in a

25 litre

flask at

27 ° C

. The initial amount of

{AB}_{2}

was

1

mole and the equilibrium pressure was

1.9 atm

. The value of

K_{p}

x \times 10^{- 2}

. The value of

x

is (Integer answer)

[R = 0.08206 {dm}^{3} atm K^{- 1} {mol}^{- 1}]

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

Graph of a reversible process;

$N_{2} + 3 H_{2} \overset{}{⇌} 2 {NH}_{3} + Heat$

is given. Analyse the graph and answer the following question.

Question Image

Identify the part of the graph which represents the forward reaction

[ OA, BA, AC]

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For

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

the
observed pressure for the reaction mixture in equilibrium is

1.12 atm

106 ° C

. What is the value of

K_{p}

for the reaction?

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction

A_{(g)} ⇌ B_{(g)} + C_{(g)}, A

33 %

dissociated at a total pressure

P .

The correct relation between

P

and

K_{p}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

Using the data provided, find the value of equilibrium constant for the following reaction at $298 K$ and $1$ atm pressure. ${NO}_{(g)} + \frac{1}{2} O_{2} (g) ⇌ {NO}_{2} (g)$
$Δ_{f} H^{0} ({NO}_{(g)}) = 90 .4 kJ . {mol}^{- 1}$

$Δ_{f} H^{0} ({NO}_{2} (g)) = 32 .48 kJ \cdot {mol}^{- 1}$

${ΔS}^{\circ} at 298 K = - 70 .8 J \cdot K^{- 1} \cdot {mol}^{- 1}$

$antilog (0 .50) = 3162$

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

60 ° C

, dinitrogen tetroxide is fifty percent dissociated. Find its standard free energy change at this temperature and one atmosphere. [ Given:

\log 1.33 = 0.1239

]

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

20 litre

container at

400 K

contains

{CO}_{2} (g)

at pressure

0.4 atm

and an excess of

SrO

(neglect the volume of solid

SrO

). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of

{CO}_{2}

attains its maximum value, will be:

(Given that : {SrCO}_{3} (s) ⇌ SrO (s) + {CO}_{2} (g), K_{p} = 1 .6 atm)

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

What are the values of

\frac{K_{p}}{K_{c}}

for the following reactions at

300 K

respectively?

(At

300 K, RT = 24 .62 {dm}^{3} atm {mol}^{- 1}

)

N_{2} (g) + O_{2} (g) ⇌ 2 NO (g); \frac{K_{p}}{K_{c}} = x_{1}

N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g); \frac{K_{p}}{K_{c}} = x_{2}

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); \frac{K_{p}}{K_{c}} = x_{3}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

The equilibrium constant for the reaction is

P_{4} (s) + 50_{2} (g) ⇌ P_{4} 0_{10} (s)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

Which one of the following is NOT an example of heterogeneous equilibrium?

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction

$H_{2 (g)} + {CO}_{2 (g)} ⇌ {CO}_{(g)} + H_{2} O_{(g)},$ if the initial concentration of $[H_{2}] = [{CO}_{2}] = 1 M$ and $x$ moles $/ L$ of $H_{2}$ is consumed at equilibrium, the correct expression of $K_{P}$ is.

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

Among the following, the correct statement about the chemical equilibrium is.

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For a reaction at equilibrium

$A (g) ⇌ B (g) + \frac{1}{2} C (g)$

the relation between dissociation constant $(K)$ , degree of dissociation $(α)$ and equilibrium pressure $(p)$ is given by :

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

A sample of

HI (g)

is placed in a flask at a pressure of

0.2 atm .

At equilibrium, partial pressure of

HI (g)

0.04 atm .

What is

Kp

for the given equilibrium ?

2 HI (g) ⇌ H_{2} (g) + I_{2} (g)

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

4.0

moles of argon and

5.0

moles of

{PCl}_{5}

are introduced into an evacuated flask of

100

litre capacity at

610 K

. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be

6.0 atm

. The

K_{p}

for the reaction is [Given :

R = 0.082 L

atm

K^{- 1} {mol}^{- 1}

]

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction

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

, if

K_{P} = K_{C} {(RT)}^{x}

where the symbols have usual meaning then the value of

x

is:
(assuming ideality)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the non-stoichiometry reaction,

2 A + B \to C + D

, the following kinetic data were obtained in three separate experiments, all at

298 K

Initial Concentration (A)	Initial Concentration (B)	Initial rate of formation of C $({mol L}^{-} S^{-})$
$0.1 M$	$0.1 M$	$1.2 \times 1 0^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 1 0^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 1 0^{- 3}$

The rate law for the formation of

C

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

Graph of a reversible process,

Question Image

is given. Analyse the graph and answer the following question.

Question Image

From the given statements, select the correct ones regarding chemical equilibrium.

(i0 The chemical equilibrium is 'static' at the molecular level.

(ii) Both reactants and products co-exist.

(iii) The rates of forward reaction and backward reactions are equal.

(iv) Chemical equilibrium is attained in an open system.

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

There are two statements, one labelled as Assertion (A) and the other as Reason (R). Examine both the statements carefully and mark the correct choice.

(A)

At equilibrium, the mass of each of the reactants and products remains constant.

(R)

At equilibrium, the rate of forward reaction is equal to the rate of backward reaction.

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the equilibrium

A ⇌ B

, the variation of the rate of the forward (a) and reverse (b) reaction with time is given by:

Explain homogeneous equilibrium with the help of an example.

Important Questions on Equilibrium

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