The rate expression for the reaction between H2O2 and KI is: rate = k[H2O2]m [KI]n where: k = rate constant m = order of reaction with respect to H2O2 n = order of reaction with respect to KI Table 2: Molarity of H2O2 and KI and Reaction Rate Trial H2O2 Concentration, M KI Concentration, M Reaction Rate (Reciprocal Slope) 1 0.29 M 0.40 M 14.08 2 0.29 M 0.20M 25 3 0.023 M 0.40 M 20 Order with respect to H2O2: -0.138 Order with respect to KI: -0.828 Rate constant value Trial 1: 5.84 Trial 2: 5.55 Trial 3: 5.56 Average: 5.6 -Please help me with this part, please 1. Should the rate constant (k) be the same for all three trials in this experiment? Explain your answer. 2.Write the complete rate law for this reaction.
The rate expression for the reaction between H2O2 and KI is:
rate = k[H2O2]m [KI]n
where: k = rate constant
m = order of reaction with respect to H2O2
n = order of reaction with respect to KI
Table 2: Molarity of H2O2 and KI and Reaction Rate
|
Trial |
H2O2 Concentration, M |
KI Concentration, M |
Reaction Rate |
|
1 |
0.29 M |
0.40 M |
14.08 |
|
2 |
0.29 M |
0.20M |
25 |
|
3 |
0.023 M |
0.40 M |
20 |
Order with respect to H2O2: -0.138
Order with respect to KI: -0.828
- Rate constant value
Trial 1: 5.84
Trial 2: 5.55
Trial 3: 5.56
Average: 5.6
-Please help me with this part, please
1. Should the rate constant (k) be the same for all three trials in this experiment? Explain your answer.
2.Write the complete rate law for this reaction.
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