The rate consnt for a reaction is measured as a function of temperature. A plot of ln k versus 1/T is linear and has s slope of -1.01 x 1-^4K. Calculate the activation energy for the reaction

Answer : The activation energy for the reaction is,

Explanation :

According to the Arrhenius equation,

Taking logarithm on both side, we get:

where,

= activation energy for the reaction

R = gas constant = 8.314 J/mole.K

T = temperature

K = rate constant

A = pre-exponential factor

The linear equation expression is:

y = mx + c

Plot of ln (K) versus (1/T) gives a straight line with a slope is equal to,

As we are given that:

Slope =

So,

Thus, the activation energy for the reaction is,

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

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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