The reaction rate of CO and NO2 in the reaction
CO(g) + NO2(g) → CO2(g) + NO(g)
is measured using the initial rates method. The results are tabulated below.
[CO] (mol/L) |
NO2 (mol/L) |
-([CO]/Δt (mol/L·s) |
||
8.00 10-4 |
5.50 10-4 |
8.40 10-8 |
||
8.00 10-4 |
7.78 10-4 |
1.68 10-7 |
||
1.60 10-3 |
5.50 10-4 |
1.68 10-7 |
Determine the rate expression and calculate the rate constant for the reaction.
Solution:
Part A) For the given reaction,
CO + NO2 = CO2 + NO
In the given data,
From trial 1 and 2, when [CO] is constant, then on increasing nealy 50 % the concentration of NO2, the rate is increased upto 100 %
Hence, order with respect to NO2 = 1/2
From trial 2 and 3, when concentration of NO2 is constant, then on douling the concentration of CO increases rate two times.
Thus, order with respect to CO = 1
Therefore, rate expression will be:
Rate = k [NO2]^1/2 [CO]
Part B) Calculation of rate constant:
From first trial, putting the values in above rate law,
Rate = k [NO2]^1/2 [CO]
8.4 x 10^-8 M s-1 = k x (5.50 x 10^-4 M)^1/2 (8.0 x 10^-4 M)
k = 8.4 x 10^-8 M s-1 / 2.35 x 10^-2 M^(-1/2) x 8.0 x 10^-4 M
k = 4.46 x 10 ^-3 M^1/2 s-1
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