from Arhenius equation
ln(K2/K1)= (Ea/R)*(1/T1-1/T2)
T1= 300KÂ Â T2= 350K K1= 21.3/M.Sec K2=3696
ln(3696/21.3)= (Ea/R)*(1/300-1/350)= (Ea/R)*0.000476
5.2= (Ea/R)*0.000476
Ea/R= 5.2/0.000476=10924.37Â Â Ea= 10924.37*8.314=
90825.21 Joules/mole
if the rate constant for the back ward reactions are K-1 at 300K
K-2 at 350 K
Keq=K1/K-1 at 300K
K-1= K1/Keq= 21.3/9*10-3=2367 /M.sec at 350 K, K-2=
3696/1.6*10-3 =2310*103
for back ward reaction ln(2310*1000/2367)= (Ea/R)*0.000476, Ea=
120228 Joules/mole
B) at 600K, forward rate constant K1 for Uncatalyzed reaction
can be calculated from Arhenius equation by Letting T1= 300K T2=
600K and Ea= 90825.21 Joules/mole
ln(K1/21.3)= (90825.21/8.314)*(1/300-1/600)=18.2 K1/21.3=
80783469 , K1= 80783469*21.3=1.721*109
similarly K=1 at 600KÂ Â ln(K-1/2367)=
(120228/8.314)*(1/300-1/600)=24
K-1= 6.94*1013
Keq= 1.721*109/6.94*1013 =2.48*10-5
