Determining reaction order: the method of initial rates
2C+3D----> E+F
exp |
(c) |
(d) |
Rate (m/s) |
1 |
2 |
2 |
10.00 |
2 |
6 |
2 |
30.00 |
3 |
1 |
1 |
1.25 |
4 |
2 |
4 |
80.00 |
Determine the order with respect to c and d and calculate the value of k
THe answer is
ANswer: Rate=k(c)^1(D)^3 K=0.675s^-1M-3
But how do you show the work
From data 1 & 2 when conc of d (2) is kept constant and conc of c is trippeled ( 2 to 6) the rate of reaction is also trippled ( 10 to 30).This shows that rate of reaction varies directly as first power of conc. Hence the order of reaction wrt c is 1.
Similarlly From data 3 & 4 when conc of d is deccreases & then increasest thhen the rate of reaction is also increases & decreases accordingly.Hence the order of reaction wrt d is 3
K = r ( rate of reaction) / [c] [d]3
= 0.1 / [2] [8] = 0.1 / 16 = 0.625 x 10-3 M-1 .
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