For the reaction, H_(2)+I_(2)overset(k_(1))underset(k_(2))hArr2HI . The rate law expression is :
For and elementary reaction 2A underset(k_(2))overset(k_(1))hArr B , the rate of disappearance of A iss equal to (a) (2k_(1))/(k_(2))[A]^(2) (b) -2k_(1)[A]^(2) + 2k_(2)[B] ( c) 2k_(1)[A]^(2) - 2k_(2)[B] (d) (2k_(1) - k_(2))[A]
A certain endothermic reaction: Ararr Product, DeltaH=+ve proceeds in a sequence of three elementary steps with the rate constants K_(1), K_(2) and K_(3) and each one having energy of activation E_(a), E_(2) and E_(3) respectively at 25^(@)C . The observed rate constant for the reaction is equal to K_(3) sqrt(K_(1)/K_(2)). A_(1), A_(2) and A_(3) are Arrhenius parameters respectively. For a reversible reaction, A underset(K_(2))overset(K_(1))(hArr) B, DeltaH=q , if perexponential factors are same. The correct relation is:
Mechanism of the reaction is: A overset(k_(1))rarrB, 2Aoverset(k_(2))rarr C + D What is (-d[A])/(dt) ?
In a reversible reaction 2NO_(2)underset(k_(2))overset(k_(1))iffN_(2)O_(4) , the rate of disappearance of NO_(2) is equal to
For the reaction , N_2O_4(g)underset(K_2)overset(K_1)hArr2NO_2(g) , the rate of disappearance of NO_2 will be
A proposed mechanism for a reaction ArarrB is A underset(k_(2))overset(k_(1))hArr C " " C underset(k_(4))overset(k_(3))hArr B Determine the expresison for the equilibrium constant for the overall reaction in terms of the rate constants.
