Determine the rate law and the value of k for the following reaction using the data provided.
S2O82-(aq)+3I-(aq) --------> 2SO42-(g)+I3-(aq)
[S2O82-]i (M) [I-]i (M) Initial Rate (M-1s-1)
0.30 0.42 4.54
0.44 0.42 6.65
0.44 0.21 3.33
Answer is Rate = 36 M-1s-1 [S2O82-] [I-]
Please show work
Given that the reaction is,
S2O8 2-(aq)+3I-(aq) --------> 2SO4 2-(g)+I3-(aq)
Let us assume,
Rate = K [S2O8 2-]^x [I-]^y
From 1st data provided in the data table,
4.54 = K (0.30)^x (0.42)^y ............(1)
From the second data
6.65 = K (0.44)^x (0.42)^y ............(2)
Dividing equation (2) by (1) we get
1.465 = (1.466)^x
=> x = 1
From the 3rd data in the data table,
3.33 = K (0.44)^x (0.21)^y ............(3)
Dividing equation (2) by equation (3) we get
2 = (2)^y
=> y = 1
Therefore,
Rate = K [S2O8 2-] [I-]
Now from equation (1)
4.54 = K (0.30) (0.42)
=> K = 36 M^-1 s^-1
=> Rate = 36 M-1s-1 [S2O82-] [I-]
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