The rate and mechamical reaction are studied in chemical kinetics. The elementary reactions are single step reaction having no mechanism. The order of reaction and molecularity are same for elementary reactions. The rate of forward reaction `aA + bBrarr cC+dD` is given as:
`rate =((dx)/(dt))=-1/a(d[A])/(dt)=-1/b(d[B])/(dt)=1/c(d[C])/(dt)=1/d(d[D])/(dt)` or expression can be written as : rate `=K_(1)[A]^(a)[B]^(b)-K_(2)[C]^(c )[D]^(d)`. At equilibrium, rate =`0`. The constants `K, K_(1), K_(2)` are rate constants of respective reaction. In case of reactions governed by two or more steps reaction mechanism, the rate is given by the slowest step of mechanism.
For a hypothetical reaction `aA+bBrarr` Product, the rate law is: rate `=K[A]^(x)[B]^(y)`, then:
A. (a) `(a+b)=(x+y)`
B. (b) `(a+b) lt (x+y)`
C. (c ) `(a+b) gt (x+y)`
D. (d) Any of these
