Home
Class 12
CHEMISTRY
Hydrogen iodide is injected into a conta...

Hydrogen iodide is injected into a container at `458^(@)C`. Certain amount of HI dissociates to `H_(2)` and `I_(2)` At equilibrium, concentration of HI is found to be `0.421M` while `[H_(2)]` and `[I_(2)]` each equal to `6.04xx10^(-2)M`, at `458^(@)C`. Calculate the value of the equilibrium constant of the dissociation of HI at the same temperature.

Text Solution

Verified by Experts

The correct Answer is:
`K_(c)=0.06xx10^(-2)`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM - II

    NCERT BANGLISH|Exercise SELF EVALUATION (C. Answer not exceeding 60 words)|3 Videos

  • CARBOXYLIC ACIDS

    NCERT BANGLISH|Exercise SELF EVALUATION((C) Answer not exceeding sixty words :)|10 Videos

  • CHEMICAL KINETICS-II

    NCERT BANGLISH|Exercise SELF EVALUATION ((D) Solve the problems :)|7 Videos

Similar Questions

Explore conceptually related problems

The standard reduction potential of the reaction, 2H_(2)O+2e rarr H_(2)+2OH^(-) is -0.8277V at 25^(@)C . Find the value of the equilibrium constant of the reaction 2H_(2)Orarr H_(3)O^(+)+OH^(-) at the same temperature.

At a particular temperature and 0.50 atm pressure, NH_(3)(g) and some amount of solid NH_(4)HS are present in a closed container. Solid NH_(4)HS dissociates to give NH_(3)(g) and H_(2)S(g) . At equilibrium, the total pressure of the reaction-mixture is found to be 0.84 atm. find the value of equilibrium constant of this reaction at that temperature.

For the equilibrium 2NOCl_((g))hArr2NO_((g))+Cl_(2(g)) the value of the equilibrium constant K_(c) is 3.75xx10^(-6) at 790^(@)C . Calculate K_(p) for this equilibrium at the same temperature.

Dissociation equilibrium constant of HI is 2.06xx10^(-2) at 458^(@)C . At equilibrium, concentrations of HI and I_(2) are 0.36M and 0.15M respectively. What is the equilibrium concentration of H_(2) at 458^(@)C .

K_c for the synthesis of HI(g) from H_2(g) and I_2(g) is 50 The degree of dissociation of HI is

2 moles of PCl_5 were heated at 327^@C in a 2 litre flask. It was found that 40% of PCl_5 dissociates to give PCl_3 and Cl_2 at equilibrium. Calculate the equilibrium constant for the dissociation of PCl_5 at equilibrium.

A 2L flask contains 0.4 g O_(2) and 0.6 g H_(2) at 100^(@)C . Calculate the total pressure of the gas mixture in the flask.

In the reaction, H_(2)(g)+I_(2)(g)hArr 2HI(g) , the value of equilibrium constant (K_(P)) changes with change in _____.

At 540, the equilibrium constant K_(p) for PCl_(5) dissociation equilibrium at 1.0 atm 1.77 atm. Calculate equilibrium constant in molar concentration (K_(c)) at same temperature and pressure.