The equilibrium constant for the reaction $H_{2} (g () + I_{2} (g) ⇌ 2 H I (g)$ is 50 at 500 K. In presence of suitable catalyst, equilibrium is attained four times faster. The equilibrium constant of the reaction at 500 K in the presence of catalyst should be-

Question

The equilibrium constant for the reaction $H_{2} (g () + I_{2} (g) ⇌ 2 H I (g)$ is 50 at 500 K. In presence of suitable catalyst, equilibrium is attained four times faster. The equilibrium constant of the reaction at 500 K in the presence of catalyst should be-

Answer 1

When a catalyst is present, the equilibrium is achieved faster but its magnitude remains unaffected. Thus the value of the equilibrium constant in presence of a catalyst is same as in absence of catalyst. i.e., 50.

Answer 2

When a catalyst is present, the equilibrium is achieved faster but its magnitude remains unaffected. Thus the value of the equilibrium constant in presence of a catalyst is same as in absence of catalyst. i.e., 50.

The equilibrium constant for the reaction $H_{2} (g () + I_{2} (g) ⇌ 2 H I (g)$ is 50 at 500 K. In presence of suitable catalyst, equilibrium is attained four times faster. The equilibrium constant of the reaction at 500 K in the presence of catalyst should be-

200

$4 \times 1 0^{4}$

50

83.6

Answer

When a catalyst is present, the equilibrium is achieved faster but its magnitude remains unaffected. Thus the value of the equilibrium constant in presence of a catalyst is same as in absence of catalyst. i.e., 50.

Practice important Questions

Chemical Equilibrium II

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For $N H_{4} H S (s) ⇌ N H_{3} (g) + H_{2} S (g)$ the observed,pressure for reaction mixture in equilibrium is 1.12 atm at $10 6^{0} C$ .

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For the following endothermic equilibrium established by dissociation of $N H_{4} H S$ to its components::

The equilibrium constant for the reaction $C a C O_{3} (s) ⇋ C a O (s) + C O_{2} (g)$ is:

At $1127 K$ and $1 a t m$ pressure, a gaseous mixture of $C O$ and $C O_{2}$ in equilibrium with solid carbon has $90.55 %$ of $C O$ by mass.

$C_{(s)} + C O_{2 (g)} ⇌ 2 C O_{(g)}$

Calculate $K_{c}$ for the reaction at the above temperature.

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The equilibrium constant for the reaction H2​(g()+I2​(g)⇌2HI(g) is 50 at 500 K. In presence of suitable catalyst, equilibrium is attained four times faster. The equilibrium constant of the reaction at 500 K in the presence of catalyst should be-

200

4×104

50

83.6

When a catalyst is present, the equilibrium is achieved faster but its magnitude remains unaffected. Thus the value of the equilibrium constant in presence of a catalyst is same as in absence of catalyst. i.e., 50.

Practice important Questions

Chemical Equilibrium II

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What , if anything can be said about the magnitude of the equilibrium constant K for the following equilibrium ?

A schematic plot in In Keq​ versus inverse of temperature for a reaction is shown below the reaction must be Exothermic Endothermic

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For NH4​HS(s)⇌NH3​(g)+H2​S(g) the observed,pressure for reaction mixture in equilibrium is 1.12 atm at 1060C. What is the value of KP​ for the reaction?

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The equilibrium constant for the reaction CaCO3​(s)⇋CaO(s)+CO2​(g) is:

At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO2​ in equilibrium with solid carbon has 90.55% of CO by mass. C(s)​+CO2(g)​⇌2CO(g)​ Calculate Kc​ for the reaction at the above temperature.

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Take Toppr Scholastic Test for Aptitude and Reasoning

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The equilibrium constant for the reaction $H_{2} (g () + I_{2} (g) ⇌ 2 H I (g)$ is 50 at 500 K. In presence of suitable catalyst, equilibrium is attained four times faster. The equilibrium constant of the reaction at 500 K in the presence of catalyst should be-

$4 \times 1 0^{4}$

What , if anything can be said about the magnitude of the equilibrium constant $K$ for the following equilibrium ?

A schematic plot in In $K_{e q}$ versus inverse of temperature for a reaction is shown below the reaction must be
Exothermic
Endothermic

For $N H_{4} H S (s) ⇌ N H_{3} (g) + H_{2} S (g)$ the observed,pressure for reaction mixture in equilibrium is 1.12 atm at $10 6^{0} C$ .

What is the value of $K_{P}$ for the reaction?

For the following endothermic equilibrium established by dissociation of $N H_{4} H S$ to its components::

The equilibrium constant for the reaction $C a C O_{3} (s) ⇋ C a O (s) + C O_{2} (g)$ is:

At $1127 K$ and $1 a t m$ pressure, a gaseous mixture of $C O$ and $C O_{2}$ in equilibrium with solid carbon has $90.55 %$ of $C O$ by mass.

$C_{(s)} + C O_{2 (g)} ⇌ 2 C O_{(g)}$

Calculate $K_{c}$ for the reaction at the above temperature.