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11th
Chemistry
Equilibrium
Homogeneous and Heterogeneous Equilibria
$Heterogeneous Equilibrium$

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Heterogeneous Equilibrium

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Heterogeneous equilibrium - definition

In an equilibrium, the reactants and the products are present in two or more that two phases, it is called a heterogeneous equilibrium.

C a C O_{3} (s) ⇋ C a O (s) + C O_{2} (g)

Expression for equilibrium constant - definition

a A (g) + b B (g) ⇋ c C (g) + d D (g)

K_{p} = \frac{p _{A}^{a} p _{B}^{b}}{p _{C}^{c} p _{D}^{d}}

K_{c} = \frac{A ^{a} B ^{b}}{C ^{c} D ^{d}}

Units of equilibrium constant - definition

K_{c} = (m o l L^{- 1})^{Δ n}

K_{c} = (a t m o r b a r)^{Δ n}

where,

Δ n = n_{p r o d u c t} - n_{r e a c t a n t}

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Class 11 Engineering - Homogeneous and Heterogeneous Equilibria

Related Concepts

Homogeneous Equilibrium

ExampleDefinitionsFormulaes

Determine the silver ion concentration in a $0.2 M$ solution of $[A g (N H_{3})_{2}] N O_{3}$ .
$A g (N H_{3})_{2}^{+} ⇌ A g^{+} + 2 N H_{3}$
$K_{d i s s .} = \frac{[ A g ^{+} ] [ N H _{3} ] ^{2}}{[ A g ( N H _{3} ) _{2}^{+} ]} = 6.8 \times 10^{- 8}$

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Pure liquids and solids can be ignored while writing the equilibrium constant expression for heterogeneous equilibria.

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In the reaction $C (s) + C O_{2} (g) ⇌ 2 C O (g),$ the equilibrium pressure is $12 a t m$ . If $50$ % of $C O_{2}$ reacts till equilibrium then $K_{p}$ will be :

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Solid ammonium carbamate dissociated into $N H_{3}$ and $C O_{2}$ as : $N H_{4} C O O N H_{2} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)$ . The total pressure at equilibrium is 0.225 atm. $K_{p}$ is $X \times 10^{- 3} a t m^{3}$ . $1000 X$ is__________.

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The value of $K$ does not depend upon pressure.

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Partial pressure of $A, B, C$ and $D$ on the basis of gaseous system at equilibrium $A + 2 B ⇌ C + 3 D$ are $A = 0.20; B = 0.10; C = 0.30$ and $D = 0.50 a t m$ .
The numerical value of equilibrium constant is-

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The unit of equilibrium constant $K$ for the reaction $A + B ⇌ C$ would be

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Give the units of $K_{c}$ for the formation of 1 mole of $N H_{3}$ from its constituents.

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One mole of A and 2 moles of B are allowed to react in a 0.5 lit flask. What is the value of $K_{c}$ ? if at equilibirum, 0.4 moles of C is formed in the reaction.
$A + 2 B \Leftrightarrow C + 2 D$

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In the reaction $2 P (g) + Q (g) ⇌ 3 R (g) + S (g)$ . If $2$ moles each of P and Q taken initially in a $1$ litre flask. At equilibrium which is true?

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Heterogeneous equilibrium - definition

Expression for equilibrium constant - definition

Units of equilibrium constant - definition

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Related Concepts

Homogeneous Equilibrium

Related questions

Determine the silver ion concentration in a 0.2M solution of [Ag(NH3​)2​]NO3​. Ag(NH3​)2+​⇌Ag++2NH3​ Kdiss.​=[Ag(NH3​)2+​][Ag+][NH3​]2​=6.8×10−8

Pure liquids and solids can be ignored while writing the equilibrium constant expression for heterogeneous equilibria.

In the reaction C(s)+CO2​(g)⇌2CO(g), the equilibrium pressure is 12 atm. If 50% of CO2​ reacts till equilibrium then Kp​ will be :

Solid ammonium carbamate dissociated into NH3​ and CO2​ as : NH4​COONH2​(s)⇌2NH3​(g)+CO2​(g). The total pressure at equilibrium is 0.225 atm. Kp​ is X×10−3atm3. 1000X is__________.

The value of K does not depend upon pressure.

Partial pressure of A,B,C and D on the basis of gaseous system at equilibrium A+2B⇌C+3D are A=0.20;B=0.10;C=0.30 and D=0.50atm. The numerical value of equilibrium constant is-

The unit of equilibrium constant K for the reaction A+B⇌C would be

Give the units of Kc​ for the formation of 1 mole of NH3​ from its constituents.

One mole of A and 2 moles of B are allowed to react in a 0.5 lit flask. What is the value of Kc​? if at equilibirum, 0.4 moles of C is formed in the reaction. A+2B⇔C+2D

In the reaction 2P(g)+Q(g)⇌3R(g)+S(g). If 2 moles each of P and Q taken initially in a 1 litre flask. At equilibrium which is true?

Determine the silver ion concentration in a $0.2 M$ solution of $[A g (N H_{3})_{2}] N O_{3}$ .
$A g (N H_{3})_{2}^{+} ⇌ A g^{+} + 2 N H_{3}$
$K_{d i s s .} = \frac{[ A g ^{+} ] [ N H _{3} ] ^{2}}{[ A g ( N H _{3} ) _{2}^{+} ]} = 6.8 \times 10^{- 8}$

In the reaction $C (s) + C O_{2} (g) ⇌ 2 C O (g),$ the equilibrium pressure is $12 a t m$ . If $50$ % of $C O_{2}$ reacts till equilibrium then $K_{p}$ will be :

Solid ammonium carbamate dissociated into $N H_{3}$ and $C O_{2}$ as : $N H_{4} C O O N H_{2} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)$ . The total pressure at equilibrium is 0.225 atm. $K_{p}$ is $X \times 10^{- 3} a t m^{3}$ . $1000 X$ is__________.

The value of $K$ does not depend upon pressure.

Partial pressure of $A, B, C$ and $D$ on the basis of gaseous system at equilibrium $A + 2 B ⇌ C + 3 D$ are $A = 0.20; B = 0.10; C = 0.30$ and $D = 0.50 a t m$ .
The numerical value of equilibrium constant is-

The unit of equilibrium constant $K$ for the reaction $A + B ⇌ C$ would be

Give the units of $K_{c}$ for the formation of 1 mole of $N H_{3}$ from its constituents.

One mole of A and 2 moles of B are allowed to react in a 0.5 lit flask. What is the value of $K_{c}$ ? if at equilibirum, 0.4 moles of C is formed in the reaction.
$A + 2 B \Leftrightarrow C + 2 D$

In the reaction $2 P (g) + Q (g) ⇌ 3 R (g) + S (g)$ . If $2$ moles each of P and Q taken initially in a $1$ litre flask. At equilibrium which is true?