(i) In an iodine-clock involving peroxide: H2O2 (aq) +2I- (aq) + 2H+(aq) → 2H2O(l) + I2 (aq) The rate law has been determined to be: rate = k [H2O2][I-] with k= 0.658 L/Ms at 250C. If [I-] = 0.5, [H2O2]=0.25 and pH=5 what is the rate of reaction? (ii) In “peroxide clock” reaction above what is the rate of loss of I- ?
(i) In an iodine-clock involving peroxide: H2O2 (aq) +2I- (aq) + 2H+(aq) → 2H2O(l) + I2 (aq) The rate law has been determined to be: rate = k [H2O2][I-] with k= 0.658 L/Ms at 250C. If [I-] = 0.5, [H2O2]=0.25 and pH=5 what is the rate of reaction? (ii) In “peroxide clock” reaction above what is the rate of loss of I- ?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.5: Temperature And Reaction Rate: The Arrhenius Equation
Problem 11.9E: The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the...
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(i) In an iodine-clock involving peroxide:
H2O2 (aq) +2I- (aq) + 2H+(aq) → 2H2O(l) + I2 (aq)
The rate law has been determined to be: rate = k [H2O2][I-] with k= 0.658 L/Ms at 250C.
If [I-] = 0.5, [H2O2]=0.25 and pH=5 what is the
(ii) In “peroxide clock” reaction above what is the rate of loss of I- ?
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