Areaction between substances y and z is
by
y2 + z2 > 2yz
the rate constant obeys the arrhenius equation. at 435.
k
the rate constant is k = 2.95 e-03 l/mol-s and a = 3.00 e+10
l/mol-s
what is the activation energy (kj/mol) for
thisreaction?

Answer : The value of activation energy for this reaction is 108.318 kJ/mol

Explanation :

The Arrhenius equation is written as:

Taking logarithm on both the sides, we get:

            ............(1)

where,

k = rate constant  =

Ea = activation energy  = ?

T = temperature = 435 K

R = gas constant  = 8.314 J/K.mole

A = pre-exponential factor  =

Now we have to calculate the value of rate constant by putting the given values in equation 1, we get:

Therefore, the value of activation energy for this reaction is 108.318 kJ/mol

diaria maybe go see a doctor about that