Home
Class 11
CHEMISTRY
For the reaction 2NOCl(g) hArr 2NO(g)+Cl...

For the reaction `2NOCl(g) hArr 2NO(g)+Cl_(2)(g)`, the equilibrium constant is `2.8xx10^(-5)` at `300 K` and `7.0xx10^(-1)` at `400 K`. What is the activation energy for the reaction?

Text Solution

AI Generated Solution

To find the activation energy (Ea) for the reaction \(2NOCl(g) \rightleftharpoons 2NO(g) + Cl_2(g)\), we can use the Arrhenius equation in its integrated form. The equation is given as: \[ \log\left(\frac{k_2}{k_1}\right) = -\frac{E_a}{2.303R} \left(\frac{1}{T_2} - \frac{1}{T_1}\right) \] Where: - \(k_1\) is the equilibrium constant at temperature \(T_1\) ...
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY ENGLISH|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

The equilibrium constant of a reaction at 298 K is 5 xx 10^(-3) and at 1000 K is 2 xx 10^(-5) What is the sign of triangleH for the reaction.

For the equilibrium 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) the value of the equilibrium constant, K_(c) is 3.75 xx 10^(-6) at 1069 K . Calcualate the K_(p) for the reaction at this temperature?

For the reaction: NOCl(g) hArr 2NO(g) +Cl_(2)(g), K_(c) at 427^(@)C is 2xx10^(6) L mol^(-1) . The value of K_(p) is

For the reaction, 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) Calculate the standard equilibrium constant at 298 K . Given that the value of DeltaH^(ɵ) and DeltaS^(ɵ) of the reaction at 298 K are 77.2 kJ mol^(-1) and 122 J K^(-1) mol^(-1) .

For the reaction: 2NOCl(g) hArr 2NO(g) +Cl_(2)(g), K_(c) at 427^(@)C is 3xx10^(-6) L mol^(-1) . The value of K_(p) is

For the reactions, CO(g) +Cl_2( g) hArr COCl_2(g), " the " (K_P)/(K_c) is equal to

The equilibrium constants for A_2 (g) hArr 2A(g) at 400 k and 600 k are 1xx 10^(-8) and 1 xx 10^(-2) respectively . The reaction is

For the reaction N_2(g) +O_2( g) hArr 2NO(g), the equilibrium constant is K1 and for reaction 2NO(g) +O_2(g) hArr 2NO_2(g) . equilibrium constant is K2 What is K for the reaction NO_2(g) hArr (1)/(2) N_2(g) + O_2(g)