1.

(a)The rate constants of a reaction at 500 K and 700 K are 0.02 s^(-1) and 0.07 s^(-1) respectively. Calculate the value of Ea. (b) Under what condition a bimolecular reaction behaves kinetically first order reaction ?

Answer»

SOLUTION :(a)Accordingtoarrheniusequation
`log(K_2) /(k_1) =(E_(Act ))/( 2.303 R) [(T_2 -T_1)/(T_1 T_2)]`
`(K_2)/(K_1) = ( 0.07 )/( 0.02)=7/2`
`T_2 = 70 K`
`T_1 = 500 K`
`R=8.314JK^(-1) Mol^(-1)`
` thereforelog (7)/(2)= (E_(a))/(2.303 xx (8.314 )/( 1000 ) )[ (700 -500 )/( 700 xx 500 )]`
`E_a= log(7 )/(2)xx ( 2.303 xx 8.314 )/( 1000 ) xx (7000 xx 500 )/( 200 )`
`=( 0.5441 xx 2.303 xx 8.314 xx 700 xx 500)/( 1000 xx 200 )`
`=18.23 KJ mol^(-1)`
(b)Thisis possibleonlywhen theone of the reactionis PRESENT inlargeexcess .


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