Home
Class 11
CHEMISTRY
For the dissociation reaction N(2)O(4)...

For the dissociation reaction
`N_(2)O_(4)(g)hArr2NO_(2)(g),`
the equilibrium constant `K_(P)` is `0.120` atm at `298 K` and total pressure of system is `2` atm. Calculate the degree of dissociation of `N_(2)O_(4)`.

Text Solution

AI Generated Solution

To solve the problem of calculating the degree of dissociation of \( N_2O_4 \) in the reaction \[ N_2O_4(g) \rightleftharpoons 2NO_2(g) \] with an equilibrium constant \( K_p = 0.120 \) atm at \( 298 \, K \) and a total pressure of \( 2 \, atm \), we will follow these steps: ...
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 dissociation reaction N_(2)O_(4) (g)hArr 2NO_(2)(g) , the degree of dissociation (alpha) interms of K_(p) and total equilibrium pressure P is:

The equilibrium constant K_(p) for the reaction N_(2)O_(4)(g)hArr2NO_(2)(g) at 497^(@)C is found to be 636 mm Hg . If the pressure of the gas mixture is 182 mm , calculate the presentage dissociation of N_(2)O_(4) . At what pressure will it be dissociated?

The degree of dissociation alpha of the reaction" N_(2)O_(4(g))hArr 2NO_(2(g)) can be related to K_(p) as:

For the reaction, N_2(g) +O_2(g) hArr 2NO(g) Equilibrium constant k_c=2 Degree of association is

For the reaction N_(2)O_(4)(g)hArr2NO_(2)(g) , the degree of dissociation at equilibrium is 0.2 at 1 atm pressure. The equilibrium constant K_(p) will be

For the reaction, N_(2)O_(4)(g)hArr 2NO_(2)(g) the degree of dissociation at equilibrium is 0.l4 at a pressure of 1 atm. The value of K_(p) is

At 1000 K , a sample of pure NO_(2) gases decomposes as : 2NO_(2)(g)hArr2NO(g)+O_(2)(g) The equilibrium constant K_(P) is 156.25 atm .Analysis showns that the partial pressure of O_(2) is 0.25 atm at equilibrium .The parital pressure o f NO_(2) at equilibrium is :

In the reaction AB(g) hArr A(g) + B(g) at 30^(@)C, k_(p) for the dissociation equilibrium is 2.56xx10^(-2) atm . If the total pressure at equilibrium is 1 atm, then the percentage dissociation of AB is

For the equilibrium H_(2) O (1) hArr H_(2) O (g) at 1 atm 298 K

For the following equilibrium N_(2)O_(4)(g)hArr 2NO_(2)(g) K_(p) is found to be equal to K_(c) . This is attained when :