What is the reaction order for each reactant and the rate coefficient for the following reaction?
A + B + C B> Z
[A] (mol L- 1) | [B] (mol L-1) | [C] (mol L-1) | [v] (mol L-1 sec-1 ) |
0.01 | 0.01 | 0.1 | 3.0 x 10-2 |
0.01 | 0.02 | 0.1 | 1.2 x 10-1 |
0.02 | 0.01 | 0.1 | 1.5 x 10-2 |
0.02 | 0.01 | 0.2 | 2.1 x 10-2 |
Let the rate equation be,
rate = k[A]^x[B]^y[C]^z
with,
k = rate constant
x, y, and z are order with respect to A, B and C
consider first and and second run, concentration of [A] and [C] are same and gets cancelled out,
rate1/rate2 = 3 x 10^-2/1.2 x 10^-1 = (0.01/0.02)^y
0.25 = 0.5^y
taking log on both sides,
log(0.25) = y log(0.5)
y = 2
Now, take run 3 and 4, [A] and [B] are constant gets cancelled out,
rate3/rate4 = 1.5 x 10^-2/2.1 x 10^-2 = (0.1/0.2)^z
0.714 = 0.5^z
taking log on both sides,
log(0.714) = z log(0.5)
z = 0.5
and last taking run 1 and 3, [B] and [C] are constant and gets cancelled out,
rate1/rate3 = 3 x 10^-2/1.5 x 10^-2 = (0.01/0.02)^x
2 = 0.5^x
taking log on both sides,
x = -1
So the rate equation becomes,
rate = k[B]^2[C]^1/2/[A]
rate coefficient or rate constant,
run 1,
3 x 10^-2 = k(0.01)^2(0.1)^1/2/(0.01)
k = 3.16 x 10^-3
Get Answers For Free
Most questions answered within 1 hours.