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

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml