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1)

 The activation energy of a reaction is zero, Its rate constant at 280 K is 1.6 x 10-6 s-1 , the rate constant at 300K is 


A) 3.2×106s1

B) zero

C) 1.6×106s1

D) 1.6×105s1

Answer:

Option C

Explanation:

Key Idea: Arrhenius  equation is given as:

 logk2k1=Ea2.303R[1T11T2]

 Given,

 Activation  energy  of a reaction , EA =0

 Rate constant  , k1 =1.6 x 10-6 s-1

 Temperature  , T1 =280 K, T2 =300K

 According to Arrhenius  equation

logk21.6×106=02.303R[12801300]

logk21.6×106=0

k21.6×106=antilog0

 k21.6×106=1

     k2=1.6×106s1