The oxidation of iodide ions by arsenic acid in acidic solution occurs according to the following stoichiometry:
H3AsO4 + 3I– + 2H3O+ → H3AsO3 + I3– + 3H2O
The experimentally determined rate law for the reaction is: rate = k[H3AsO4][I–][H3O+]. What is the order of the reaction with respect to H3AsO4?
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2018-08-01 7:23 am
回答 (3)
2018-08-01 9:18 am
✔ 最佳答案
Rate law: Rate = k [H₃AsO₄] [I⁻] [H₃O⁺]The reaction with respect to H₃AsO₄ is the power of [H₃AsO₄] in the rate law.
Refer to the above rate law. The power of [H₃AsO₄] in the rate law is 1.
Hence, the order with respect to H₃AsO₄ = 1
2018-08-01 10:24 am
Order .....
I thought this looked familiar. I've already answered this question for you
https://answers.yahoo.com/question/index?qid=20180728020521AAAQAXH
The reaction is first order in each one of the three reactants.
I thought this looked familiar. I've already answered this question for you
https://answers.yahoo.com/question/index?qid=20180728020521AAAQAXH
The reaction is first order in each one of the three reactants.
2018-08-01 8:52 am
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yes you are correct. it is 1
yes you are correct. it is 1
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