The equilibrium constant K c at 298 K for the reaction A + B leftharpoons C + D is 100 . Starting with an equimolar solution with concentrations of A , B , C and D all equal to 1 M, the equilibrium concentration of D is × 10-2 M. (Nearest integer)

Question

The equilibrium constant K c at 298 K for the reaction A + B leftharpoons C + D is 100 . Starting with an equimolar solution with concentrations of A , B , C and D all equal to 1 M, the equilibrium concentration of D is × 10-2 M. (Nearest integer) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

First check direction of reversible reaction. Since Q c =([ C ][ D ]/[ A ][ B ])=1< K text eq. ⇒ reaction will

Now: K eq =100=((1+ x )(1+ x )/(1- x )(1- x )) ⇒ 100=((1+x/1-x))2 (i) 10=((1+x/1-x)) ⇒ 10-10 x=1+x ⇒ 11 x=9 ⇒ x=(9/11) (ii) -10=(1+x/1-x) ⇒ -10+10 x=1+x ⇒ -9 x=-11 ⇒ x=(11/9) arrow ' x ' cannot be more than one, therefore not valid. therefore equation concretion of ( D )=1+ x =1+(9/11)=(20/11) =1.8181=181.81 × 10-2 ≃ 182 × 10-2

Q. The equilibrium constant Kc​ at 298K for the reaction A+B⇌C+D is 100 . Starting with an equimolar solution with concentrations of A,B,C and D all equal to 1M, the equilibrium concentration of D is___ ×10−2M. (Nearest integer)

Q. The equilibrium constant $K_{c}$ at $298 K$ for the reaction $A + B ⇌ C + D$ is $100$ . Starting with an equimolar solution with concentrations of $A, B, C$ and $D$ all equal to $1 M$ , the equilibrium concentration of $D$ is___ $\times 1 0^{- 2} M$ . (Nearest integer)