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asad345 asad345
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3 years ago
The oxidation of Cr3+ to CrO42– can be accomplished using Ce4+ in a buffered solution. The following data were obtained:
 
Relative
Initial Rate
[Ce4+]0
[Ce3+]0
[Cr3+]0
 
1
2.0 × 10–3
1.0 × 10–2
3.0 × 10–2
 
2
4.0 × 10–3
2.0 × 10–2
3.0 × 10–2
 
4
4.0 × 10–3
1.0 × 10–2
3.0 × 10–2
 
16
8.0 × 10–3
2.0 × 10–2
6.0 × 10–2

​

Determine the order in the rate law of the species Cr3+.

 
Reference: Ref 12-7

​

​



▸ 1

▸ 2

▸ 3

▸ –1

▸ –2
Textbook 
Chemistry: An Atoms First Approach

Chemistry: An Atoms First Approach


Edition: 3rd
Authors:
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IlovesushiIlovesushi
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#2
A year ago
let the rate (r)= K[Ce+4]a [ Ce+3]b [Cr+3]c, a, b and c are orders with respect to Ce+4, Ce+3 and Cr+3 respectively. K is the rate constant

from 2nd data point, 2= K[ 4*10-3]a* [ 2*10-2]b* [3*10-2]c , (1)

from the 3rd data point, 4= K[ 4*10-3]a* [ 1*10-2]b* [3*10-2]c , (2)

Eq.2/Eq.1= 2= (1/2) b= 2-b= 2 , b=-1, the order of reaction with respect to Ce+3.
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