For the dissociation reaction `N_(2)O_($) (g)hArr 2NO_(2)(g)`, the degree of dissociation `(alpha)`interms of `K_(p)` and total equilibrium pressure P is:
For a reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g))
At certain temperature compound AB_(2)(g) dissociates accoring to the reacation 2AB_(2)(g) hArr2AB (g)+B_(2)(g) With degree of dissociation alpha Which is small compared with unity, the expression of K_(p) in terms of alpha and initial pressure P is :
For the reaction CO(g)+Cl_(2)(g)hArrCOCl_(2)(g) the value of (K_(c)/(K_(P))) is equal to :
The equilibrium constant K_(p) for the following reaction is 4.5 N_(2)O_(4)(g)hArr2NO_(2)(g) What would be the average molar mass ("in"g//mol) of an equilibriumm mixture of N_(2)O)(4) and NO_(2) formed by the dissociation of pure N_(2)O_(4) at a jtotal pressure of 2 atm ?
For the reaction N_(2)(G)+3H_(2)(g)hArr2NH_(3)(g),Delta=-93.6KJmol^(-1) The number of moles o fH_(2) at equilibrium will increase If :
For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with
For the reaction 2NO_(2)(g)+(1)/(2)O_(2)(g)hArrN_(2)O_(5)(g) if the equilibrium constant is K_(p) , then the equilibrium constant for the reaction 2N_(2)O_(5)(g)hArr4NO_(2)(g)+O_(2)(g) would be :
Consider the reaction 2CO(g)+O_(2)(g)hArr2CO_(2)(g)+Heat Under what conditions shift is undetminable ?
For the reversible reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) at 500^(@)C , the value of K_(p) is 1.44xx10^(-5) when the partial pressure is measured in atmosphere. The corresponding value of K_(c) with concentration in mol L^(-1) is
For the reaction H_(2)(g)+CO(g)hArrCO(g)+H_(2)O(g), if the initial concentration of [H_(2)]=[CO_(2)] and x moles /litres of hydrogen is consummed at equilibrium , the correct expression of K_(p) is :
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
