In a reversible reaction `2NO_(2)underset(k_(2))overset(k_(1))iffN_(2)O_(4)`, the rate o

For the reversible reaction equilibrium is N_(2)(g)+O_(2)(g)underset(k_(2))overset(k_(1))(hArr)2NO(g) C_(0)=Ce^(-2.1xx10^(3)) for the forward and C_(0)^(')=C^(')e^(-4.2xx10^(-4t)) for the backward reaction, hence, K_(c) for the above equilibrium is (both forward and backward reactions are first order reactions )

For an elementary chemical reaction, A_(2) underset(k_(-1))overset(k_(1))(hArr) 2A , the expression for (d[A])/(dt) is

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

For a reversible reaction (first order in both directions) Aunderset(k_(1))overset(k_(2))hArrB k_(1) and k_(2) are the rate constant. If equlibrium constant (K) is greater than unity, then :

The mechanism of the reaction 2NO + O_(2) rarr 2NO_(2) is NO + NO underset(k_(-1))overset(k_(1))hArr N_(2)O_(2) ("fast") N_(2)O_(2) + O_(2) overset(k_(2))rarr 2NO_(2) (slow) The rate constant of the reaction is

2SO_(2) + O_(2) underset(k_(2))overset(k_(1))hArr 2SO_(3) What are the expresison for the rate law of the forward and backward reactions?

Consider a system containing NO_(2) and SO_(2) in which NO_(2) is consumed in the following two parallel reactions. 2NO_(2) overset(K_(1)) to N_(2)O_(4), NO_(2) + SO_(2) overset(K_(2)) to NO + SO_(3) The rate of disappearance of NO_(2) will be equal to