Listed in the table are forward and reverse rate constants for the reaction
`2NO(g)hArrN_(2)(g)+O_(2)(g)`
`{:(,Temperature(K),k_(f)(M^(-1)s^(-1)),k_(b)(M^(-1)s^(-1))),(,1400,0.29,1.1xx10^(-6)),(,1500,1.3,1.4xx10^(-5)):}`
Select the correct statement

Forward and reverse rate constant for the reaction CO_(2)(g) + N_(2)(g) CO(g) + N_(2)O exhibit the following temperature dependence. {:("Temperature (K)",k_(f)(M^(-1)S^(-1)),k_(r)(M^(-1)s^(-1))),(1200,9.1xx10^(-11),1.5xx10^(5)),(1500,2.7xx10^(-9),2.6xx10^(5)):} Is the reaction endothermic or exothermic? Explain in terms of kinetics.

At a given temperature, the equilibrium constant for the reactions NO(g)+1//2O_(2)(g)hArr NO_(2)(g) and 2NO_(2)(g)hArr 2NO(g)+O_(2)(g) are K_(1) and K_(2) respectivel. If K_(1) is 4xx10^(-3) then K_(2) will be

The equilibrium constant, K for the reaction : 2HI (g) hArr H_(2)(g)+I_(2)(g) at room temperature is 2.85 and that of at 698 K is 1.4 xx 10^(-2) . This implies that the forward reaction is

The kinetic date for the given reaction A(g)+2B(g)overset(K)toC(g) is provided in the following table for three experiments at 300 K {:("Ex. No.","[A/M]","[B/M]","Initial rate" (M sec^(-1))),(1.,0.01,0.01,6.930xx10^(-6)),(2.,0.02,0.01,1.386xx10^(-5)),(3.,0.2,0.02,1.386xx10^(-5)):} In another experiment starting swith initial concentration of 0.5 and 1 M respectively for A and B at 300 K, find the rate of reaction after 50 minutes from the starting of edperiment (inM // sec).

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below: i. O_(3)(g) + Cl^(*)(g) to O_(2)(g) + ClO^(*) , k_(1) = 5.2 xx 10^(9) "L mol"^(-1)s^(-1) (ii) ClO^(*) (g) + O^(*)(g) to O_(2)(g) + Cl^(*), k_(II) = 2.6 xx 10^(10) L "mol"^(-1)s^(-1) The closest rate constant for the overall reaction O_(3)(g)+O^(.)(g)rarr2O_(2)(g) is : 1.4 xx 10^(20) L mol^(-1) s^(-1) , 3.1 xx 10^(10) L mol^(-1) s^(-1) , 5.2 xx 10^(9) L mol^(-1) s^(-1) , 2.6 xx 10^(10) L mol^(-1) s^(-1)

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g)hArr 2NO(g) at temperature T is 4xx10^(-4) . The vlue of K_(c ) for the reaction NO(g)hArr (1)/(2)N_(2)(g)+(1)/(2)O_(2)(g) at the same temperature is :

Identify the reaction order from each of the following rate. i) k=2.3 xx 10^(5) L mol^(-1)s^(-1) ii) k=2.3 xx 10^(5)Lmol^(-1)s^(-1) ii) k=3.1 xx 10^(-4)s^(-1)

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is