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Homogeneous and Heterogeneous Equilibria

Equilibrium

Chemistry

Class 11

Overview

2 mins read

Homogeneous Equilibrium

Heterogeneous Equilibrium

Which of the following factors will increase solubility of $N H_{3} (g) i n H_{2} O$
$N H_{3} (g) + H_{2} O (a q) ⇌ N H_{4} O H (a q)$

Four moles of $P C l_{5}$ are heated in a closed $4 d m^{3}$ container to reach equilibrium at 400K. At equilibrium, 50% of $P C l_{5}$ is dissociated. What is the value of $K_{c}$ for the dissociation of $P C l_{5}$ into $P C l_{3}$ and $C l_{2}$ at 400K?

$K_{p} = K_{c}$ for all reactions. BECAUSE

For the reaction, $C O (g) + C l_{2} (g) ⇌ C O C l_{2} (g)$ the $\frac{K _{p}}{K _{c}}$ is equal to

At $22 7^{o} C$ temperature, for the reaction $P C I_{5 (g)} + ⇄ P C I_{3 (g)} + C I_{2 (g)}$ , the value of equilibrium constant $K_{c}$ is $1.255 \times 1 0^{- 2} m o l / l i t$ . Calculate $K_{p}$ of the reaction

For a given exothermic reaction $K_{p}$ and $K^{^{'}}_{p}$ are the equilibrium constants at temperature $T_{1}$ and $T_{2}$ respectively. Assuming that heat of reaction is constant in temperature range between 183. $T_{1}$ and $T_{2}$ it is readily observed that:

Equilibrium constant for the reaction $2 N O (g) + C l_{2} (g) ⇌ 2 N O C l (g)$ is correctly given by the expression:

$lo g \frac{K _{P}}{K _{C}} + lo g R T = 0$ lis true reationship for the following reaction :-

One mole of nitrogen is mixed with 3 mole of hydrogen in a closed 3 liter vessel. 20 % of nitrogen is converted into $N H_{3}$ . Then $K_{c}$ for the $\frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ N H_{3}$

For the system $A_{(g)} + 2 B_{(} g) ⇌ C_{(g)}$ , the equilibrium concentrations are
$A = 0.06 m o l L^{- 1}$
$B = 0.12 m o l L^{- 1}$
$C = 0.216 m o l L^{- 1}$
Then $K_{c}$ for the reaction is _____.

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Homogeneous and Heterogeneous Equilibria

Overview

Homogeneous Equilibrium

Heterogeneous Equilibrium

Which of the following factors will increase solubility of NH3​(g)inH2​O NH3​(g)+H2​O(aq)⇌NH4​OH(aq)

Four moles of PCl5​ are heated in a closed 4dm3 container to reach equilibrium at 400K. At equilibrium, 50% of PCl5​ is dissociated. What is the value of Kc​ for the dissociation of PCl5​ into PCl3​ and Cl2​ at 400K?

Kp​=Kc​ for all reactions. BECAUSE

For the reaction, CO(g)+Cl2​(g)⇌COCl2​(g) the Kc​Kp​​ is equal to

At 227oC temperature, for the reaction PCI5(g)​+⇄PCI3(g)​+CI2(g)​, the value of equilibrium constant Kc​ is 1.255×10−2mol/lit. Calculate Kp​ of the reaction

For a given exothermic reaction Kp​ and K′p​ are the equilibrium constants at temperature T1​ and T2​ respectively. Assuming that heat of reaction is constant in temperature range between 183. T1​ and T2​ it is readily observed that:

Equilibrium constant for the reaction 2NO(g)+Cl2​(g)⇌2NOCl(g) is correctly given by the expression:

logKC​KP​​+logRT=0 lis true reationship for the following reaction :-

One mole of nitrogen is mixed with 3 mole of hydrogen in a closed 3 liter vessel. 20 % of nitrogen is converted into NH3​ . Then Kc​ for the 21​N2​+23​H2​⇌NH3​

For the system A(g)​+2B(​g)⇌C(g)​, the equilibrium concentrations are A=0.06 mol L−1 B=0.12 mol L−1 C=0.216 mol L−1 Then Kc​ for the reaction is _____.

Which of the following factors will increase solubility of $N H_{3} (g) i n H_{2} O$
$N H_{3} (g) + H_{2} O (a q) ⇌ N H_{4} O H (a q)$

Four moles of $P C l_{5}$ are heated in a closed $4 d m^{3}$ container to reach equilibrium at 400K. At equilibrium, 50% of $P C l_{5}$ is dissociated. What is the value of $K_{c}$ for the dissociation of $P C l_{5}$ into $P C l_{3}$ and $C l_{2}$ at 400K?

$K_{p} = K_{c}$ for all reactions. BECAUSE

For the reaction, $C O (g) + C l_{2} (g) ⇌ C O C l_{2} (g)$ the $\frac{K _{p}}{K _{c}}$ is equal to

At $22 7^{o} C$ temperature, for the reaction $P C I_{5 (g)} + ⇄ P C I_{3 (g)} + C I_{2 (g)}$ , the value of equilibrium constant $K_{c}$ is $1.255 \times 1 0^{- 2} m o l / l i t$ . Calculate $K_{p}$ of the reaction

For a given exothermic reaction $K_{p}$ and $K^{^{'}}_{p}$ are the equilibrium constants at temperature $T_{1}$ and $T_{2}$ respectively. Assuming that heat of reaction is constant in temperature range between 183. $T_{1}$ and $T_{2}$ it is readily observed that:

Equilibrium constant for the reaction $2 N O (g) + C l_{2} (g) ⇌ 2 N O C l (g)$ is correctly given by the expression:

$lo g \frac{K _{P}}{K _{C}} + lo g R T = 0$ lis true reationship for the following reaction :-

One mole of nitrogen is mixed with 3 mole of hydrogen in a closed 3 liter vessel. 20 % of nitrogen is converted into $N H_{3}$ . Then $K_{c}$ for the $\frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ N H_{3}$

For the system $A_{(g)} + 2 B_{(} g) ⇌ C_{(g)}$ , the equilibrium concentrations are
$A = 0.06 m o l L^{- 1}$
$B = 0.12 m o l L^{- 1}$
$C = 0.216 m o l L^{- 1}$
Then $K_{c}$ for the reaction is _____.