Question

For a reaction, activation energy (Eₐ) = 0 and rate constant
(k) = 3.2 × 10⁶ s⁻¹ at 300 K. What is the value of the rate
constant at 310 K
(a) 3.2 × 10⁻¹² s⁻¹ (b) 3.2 ´106 s⁻¹
(c) 6.4 × 10¹² s⁻¹ (d) 6.4 ´106 s⁻¹

Answer 1

answer : option (b) 3.2 × 10⁶ s-¹

according of Arrhenius activation energy formula,

k = Ae^{-Ea/RT}

where A is proportionality factor, k is rate constant, T is temperature in Kelvin and R is universal gas constant.

given, activation energy,(Ea) = 0

so, k = Ae^{-0/RT} = A

hence rate constant always remains same.

so, rate constant at 300K = rate constant at 310K

i.e., k = 3.2 × 10⁶ s-¹

hence, option (b) is correct choice.

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Answer 2

Answer:

option b

Explanation:

3.2 106 s

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