k(300 K) = 6*109 1/(M2 s) and the rate constant at 1000 K is
k(1000 K) = 3*1010 1/(M2 s). Calculate the Arrhenius parameters and the order of the reaction.
Need Work shown
K (300K) = 6*109 M-2 s-1
K (1000 K) = 3*1010 M-2 s-1.
From logarithm expression of Arrhenius equation
ln
= -
(
-
)
Or,
ln ( 3*1010/6*109) = -
(
-
)
Or, 1.609 = -
* ( -0.002333)
Or, Ea = (1.609 *8.314)/(0.002333)
Or, Ea = 5733 J/mole .
Again.
K = A * e- Ea/RT
At T = 300 K, K = 6*109
So, 6*109 = A * e-{5733/(8.314*300)}
Or,6*109 = A * 0.1004
Or, A = ( 6*109/0.1004) = 59.76*109 = 5.976*1010
.
Rate = K * [A]n
Or, K = Rate/[A]n
[A] is concentration of reactant.
Hence, General unit of rate constant (K)
= (M)1-n s-1.
Where , n = order of the reaction.
In the given problem
Unit is M-2s-1
So, 1-n = -2
Or, n = 1+2= 3.
Therefore , order of the reaction is 3.
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9,10,11
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