Question

a)The order of this ozone decomposition reaction is __________ order because __________.b)The rate constant for this ozone decomposition reaction is ______ (include units!)c)How many minutes will it take before half of the original ozone concentration ([O3]0) is depleted?

Answer 1

Answer:

a). Second order reaction.

b). $50.14\ Lmol^{-1}s^{-1}$

c).  $t_{1/2}=1994.41 \ h$

Explanation:

a). The order of the reaction of ozone decomposition is second order reaction.

It will be second order because the plot between the Inverse of Concentration versus Time will be a straight line.

$\frac{1}{[A]}=\frac{1}{[A_0]}+kt$

b). Calculating slope by

$y_0= 100000.000$

$y_1= 952380.952$

$\Delta y = 852380.9524$

$x_0=0E+00$

$x_1= 2E+04$

$\Delta x = 2E+04$

Slope, k = $\frac{\Delta y}{\Delta x}=50.14$

Thus we see that the slope of the curve will be rate constant.

Therefore, rate constant = $50.14\ Lmol^{-1}s^{-1}$

c). We know half life ,

$t_{1/2}=\frac{1}{k[A_0]}$

$[A_0]=0.00001 \ mol/L$

k = $50.14\ Lmol^{-1}s^{-1}$

Putting the values, we get

$t_{1/2}=\frac{1}{50.14[0.00001]}$

$t_{1/2}=1994.41 \ h$