The equilibrium constant at 298 K for a reaction, `A+B⇌C+D is 100. If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L −1 ) will be:

Options

A. 0.182
B. 0.818
C. 1.818
D. 1.182

Explanation

`Q_c=([C][D])/([A][B])=(1xx1)/(1xx1)=1`
`:'Q_cltK_c`, net reaction
`A+B Begining 1M 1M 1M 1M
Equilibrium `(1-x)M (1-M)M (1+x)M (1+x)M`
`K_c=([C][D])/([A][B])=((1+x)(1+))/((1-x)(1-x))=100`
or `((1+x)/(1-x))^2=100` or `(1+x)/(1-x)=10` or, `11x=9" or "x=0.818`
`:.[D]=(x+x)(M)=1.818(M)`