Skip to main content
Ch.14 - Chemical Kinetics

Chapter 14, Problem 13

To answer questions 13–15, refer to the mechanism: H2O21aq2 + I-1aq2¡OH-1aq2 + HOI1aq2 Slower, rate-determining HOI1aq2 + I-1aq2¡OH-1aq2 + I21aq2 Faster 2 OH-1aq2 + 2 H3O+1aq2¡4 H2O1l2 Faster Identify the catalyst and intermediate(s) in the mechanism. (LO 14.12, 14.16) (a) Catalyst = I-, intermediates = OH-, HOI (b) Catalyst = H3O+, intermediate = HOI (c) No catalyst, intermediate = I2 (d) No catalyst, intermediates = OH-, HOI

Verified Solution
Video duration:
3m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Video transcript

Hello everyone today. We have the following question. Consider the following reaction mechanism, determine the catalyst and the intermediates. So first let's define what a catalyst and what an intermediate are. So it cattle's essentially speeds up a chemical reaction and it's going to appear so a catalyst appears as a reactant and so it appears as a reactant in the first step. However, in the second step it appears as a product as a product, not necessarily the second step, but the last step. And so we can also define what an intermediate is. So an intermediate is essentially not a catalyst or product, but it's going to be some compound that ends up being canceled out. And so if you look at this equation for this chemical reaction, we can determine what the catalyst would be. So if we look closely in the first step, we have water here appearing as a reaction. And in the very last step we also have water appearing as well. So our catalyst, It's going to be water or H20. And so that gets rid of the answer choices A and B. Since we do have a catalyst next, we're going to look for our intermediate. And so that's going to involve canceling out anything that shows up on the reacting side, on the product side. So if we look at our H20. We see that it cancels out on the left here and then the last step there on the right, we also noticed how our hydroxide on the right and the first step. And then on the left. And the third step aside from that, we can also identify that we have our hipAA Cloris acid on the right here, the first step and also on the left side in the second step. And then we can conclude that there are no other similarities that are present. Until we look at our second step here and we find our hypo I. D. On the right and on the left of the 2nd and 3rd step. So we said our intermediates are things that are ending up being crossed out. So we have our hipAA Cloris acid, R. H. O. I. And we have our hydroxide. We aren't gonna count water because we've already concluded that water is our catalyst. And so the anti choice that best aligns with what we chose is going to be anti choice. See and with that we've answered the question overall. I hope this helped. And until next time.
Related Practice
Textbook Question
The gas phase decomposition of HI has the following rate law: 2 HI1g2¡H21g2 + I21g2 Rate = k3HI42 At 443 °C, k = 30.1 M-1 min-1. If the initial concentration of HI is 0.010 M, what is the concentration after 1.5 hours? (LO 14.8) (a) 6.9 * 10-3 M (b) 1.8 * 10-3 M (c) 3.6 * 10-4 M (d) 8.9 * 10-4 M
1060
views
Textbook Question
Chlorine monoxide (ClO) decomposes at room temperature according to the reaction 2 ClO1g2¡Cl21g2 + O21g2 The concentration of ClO was monitored over time, and three graphs were made:

What is the rate law for the reaction? (LO 14.9) (a) Rate = k (b) Rate = k3ClO4 (c) Rate = k3ClO42 (d) Rate = k3ClO43 M14_MCMU6230_
382
views
Textbook Question
A key reaction in the upper atmosphere is O31g2 + O1g2 ¡ 2 O21g2 For this process, the energy of activation for the forward reaction, Ea1fwd2, is 19 kJ/mol, and the enthalpy change for the reaction, ΔHrxn, is -392 kJ>mol. What is the energy of activation for the reverse reaction, Ea1reverse2? (LO 14.10) (a) 411 kJ/mol (b) 392 kJ/mol (c) 373 kJ/mol (d) 196 kJ/mol
525
views
Textbook Question

Ammonia is manufactured in large amounts by the reaction

N2(g) + 3 H2(g) → 2 NH3(g)

(a) How is the rate of consumption of H2 related to the rate of consumption of N2?

118
views
Textbook Question
(b) Write the balanced reaction that corresponds to the data in the graph.

837
views
2
rank
Textbook Question

The following reaction is first order in A (red spheres) and first order in B (blue spheres): A + B → Products Rate = k[A][B]

(a) What are the relative rates of this reaction in vessels (1)–(4)? Each vessel has the same volume.

475
views
1
rank