t in seconds |
0 |
900 |
1800 |
Cone. of A |
50.8 |
19.7 |
7.62 |
Prove that the reaction is of first order of A to decompose to one-half.
For the first order reaction can given by
At t = 900 seconds,
(i)
(ii)
Since the value of k is both case is almost same thus it is first order reaction.
S.No. |
A(M) |
B(M) |
Initial rate (M) |
1. |
1.00 |
1.00 |
1.2 x 10–2 |
2. |
1.00 |
2.00 |
4.8 x 10–2 |
3. |
1.00 |
4.00 |
1.9 x 10–1 |
4. |
4.00 |
1.00 |
4.9 x 10–2 |
Assuming that rate law can be written as
Determine the value of
We have to assume that law canbe written as
Thus
or
From reaction no. (iv) and (i)
or
The order of the reaction is first order with respect to A and second order with respect to B. Overall order of the reaction is 3.
Rate = k[H2] [NO]2
The order of each reactant
Order with respect to H2 = 1
Order with respect to NO = 2.
Overall order = 1 + 2 = 3.
We have given intial concentration 2x10-3and 1x10-3.
the intial concentration equal to 2.40 x 10-4 Ms-1 and 0.60 x10-4 MS-1
Let the rate be =
From the trial (i) and (ii), we get
or
Thus reaction is of second order