For a chemical reaction `A rarr` Products, the rate of disappearance of `A` is given by:
`-(dC_(A))/(dt)=(K_(1)C_(A))/(1+K_(2)C_(A))` At low `C_(A)`, the reaction is of the …. Order with rate constant …..: `("Assume" K_(1), K_(2) "are lesser than" 1)`

For a chemical reaction Ato Products, the rate of disappearance of A is given by: (dC_(A))/(dt)=(K_(1)C_(A))/(1+K_(2)C_(A)) at low C_(A) , the reaction is of the _________order with rate constant_________(Assume K_(1), K_(2) are lesser than 1)

The rate of reaction ((dx)/(dt)) varies with nature, physical state and concentration of reactants, temperature, exposure to light and catalyst, whereas rate constant (K) varies with temperature and catalyst only. The rate constant K is given as K=Ae^(-E_(a)//RT) where A is Arrhenius parameter or pre-exponential factor and E_(a) is energy of activation. The minimum energy required for a reaction is called threshold energy and the additional energy required by reactant molecules to attain threshold energy level is called energy of activation. For a chemical reaction: Ararr Product, the rate of disappearance of A is given by: (-dC_(A))/(dt)=K_(1) (C_(A))/(1+K_(2)C_(A)) . At low C_(A) , the order of reaction and rate constants are respectively:

The rate of reaction, A + B + C rarr P is given by: r=-(d[A])/dt=K[A]^(1//2)[B]^(1//2)[C]^(1//4) . The order of the reaction is:

The rate of the reaction A+B+C to Product is given by: rate =-(d[A])/(dt)=k[A]^(1//2) [B]^(1//4) [C]^0 The order of reaction is:

The rate of the reaction A+B+C to Product is given by: rate =-(d[A])/(dt)=k[A]^(1//2) [B]^(1//4) [C]^0 The order of reaction is:

The rate of certain hypothetical reaction A+B+C rarr Products, is given by r = -(dA)/(dt) = k[A]^(1//2)[B]^(1//3)[C]^(1//4) The order of a reaction is given by

The rate of certain hypothetical reaction A+B+C rarr Products, is given by r = -(dA)/(dt) = k[A]^(1//2)[B]^(1//3)[C]^(1//4) The order of a reaction is given by

The rate of certain hypothetical reaction A+B+C rarr Products, is given by r = -(dA)/(dt) = k[A]^(1//2)[B]^(1//3)[C]^(1//4) The order of a reaction is given by