Exam1_FR_sum04[1]

4 47 50 53 56 59 1n2o5 81 109 147 200 270 357

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Unformatted text preview: ‐5.6 ‐5.9 1 / [N2O5] 81 109 147 200 270 357 A) Using the above information, determine the order of the reaction for N2O5 by graphical means. Order = _______ B) Write BOTH the differential and integrated forms of the rate law for this equation. C) Calculate k for this reaction (include units). D) What will be the concentration of [N2O5] when t= 100.0 min? #2 continued E) What will be the rate of the reaction at time = 50.0 min? F) What is the ½‐life of the reaction? 3. Consider the overall reaction: H2O2 + 3I− + 2H+ → I3− + 2H2O A) The following mechanism is proposed for this reaction: k1 (fast equilibrium, rate constants: k and k ) + H3O2+ Step 1. H2O2 + H 1 ‐1 Step 2. H3O2+ + I– H2O + HOI (slow, rate constant k2) Step 3. HOI + I– OH– + I2 (fast, rate constant k3) Step 4. OH– + H+ H2O (fast, rate constant k4) Step 5. I2 + I– I3– (fast, rate constant k5) k‐1 What would be the predicted differential rate law expression for this mechanism? B) What is the role of HOI in this mechan...
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This note was uploaded on 09/11/2013 for the course CHEM 220 taught by Professor Bates during the Spring '10 term at Skyline College.

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