The reaction of `O_(3)` with chlorine atom is given as :
`O_(3)(g)+Cl(g)rarrO_(2)(g)+ClO(g),k_(1)=5.2xx10^(9)L"mol"^(-1)sec^(-1)`
`ClO(g)+O(g)rarrCl(g)+O_(2)(g),k_(2)=2.6xx10^(10)L"mol"^(-1)sec^(-1)`
Which of theses values is closest to the rate constant of the overall reaction ?
`O_(3)(g)O(g)rarr2O_(2)(g)`

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below: O_(3)(g)+Cl^(.)rarrO_(2)(g)+ClO^(.)(g)…(i) k_(i)=5.2xx10^(9)" L mol"^(-1)s^(-1) ClO^(.)(g)+O^(.)(g)rarrO_(2)(g)+Cl^(.)(g).......(ii) k_(ii)=2.6xx10^(10)"L mol"^(-1)s^(-1) The closest rate constant for the overall reaction O_(3)(g)+O^(.)(g)rarr2O_(2)(g) is :

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 of the following reactions at 400 K are given: 2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g), K_(1)=3.0xx10^(-13) 2CO_(2)(g) hArr 2CO(g)+O_(2)(g), K_(2)=2xx10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g)+CO_(2)(g) hArr CO(g)+H_(2)O(g) is

The equilibrium constant for the following reactions at 1400 K are given. 2H_(2)O(g)hArr2H_(2)(g) + O_(2)(g) , K_(1)=2.1×x10^(-13) 2CO_(2)(g) hArr2CO(g)+O_(2)(g),K_(2) = 1.4 x× 10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g) + CO_(2)(g)hArrCO(g) + H_(2)O(g) is

For the reaction, 2NO_(2)(g) rarr 2NO(g) + O_(2)(g), K_(c) = 1.8 xx 10^(-6) "at" 185^(@)C , the value of K_(c) for the reaction NO(g) + 1/2O_(2)(g) rarr NO_(2)(g) is

For the reaction, 2NO_(2)(g) rarr 2NO(g) + O_(2)(g), K_(c) = 1.8 xx 10^(-6) "at" 185^(@)C , the value of K_(c) for the reaction NO(g) + 1/2O_(2)(g) rarr NO_(2)(g) is

The initial concentration of N_(2)O_(5) in the following first order reaction: N_(2)O_(5)(g) rarr 2NO_(2)(g)+(1)/(2)O_(2)(g) was 1.24 xx 10^(-2) mol L^(-1) at 318 K . The concentration of N_(2)O_(5) after 60 min was 0.20 xx 10^(-2) mol L^(-1) . Calculate the rate constant of the reaction at 318 K .