Consider the reaction: 2 NH 3 (aq) + OCl - (aq) → N 2 H 4 (aq) + H 2 O(l) + Cl - (aq) This three-step mechanism is proposed: NH 3 (aq) + OCl - (aq) Δk1k2 NH 2 Cl(aq) + OH- (aq) Fast NH 2 Cl(aq) + NH 3 (aq) →k3 N 2 H 5 + (aq) + Cl - (aq) Slow N 2 H 5 + (aq) + OH - (aq) →k4 N 2 H 4 (aq) + H 2 O(l) Fast a. Show that the mechanism sums to the overall reaction.

Hi everyone here we have a question asking us to identify the overall reaction for the reaction mechanism below. A. B plus C to D. Forms A C to D plus B. Fast. B plus A B forms A B to slow A C to D plus A B. To form A to B to C. To D. Fast. So let's cancel out what we can. So we have a C. To D. Here and here. So those will cancel out and then we have B here and here. So those will cancel out and then we have a. B. Two here and here. So those will cancel out. This gives us the overall reaction of to A B plus C to D. Forms a two B C to D. And that is our final answer. Thank you for watching. Bye.

Ch.14 - Chemical Kinetics

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Tro 4th Edition

Ch.14 - Chemical Kinetics

Problem 106a

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Chapter 14, Problem 106a

Consider the reaction: 2 NH₃(aq) + OCl^-(aq) → N₂H₄(aq) + H₂O(l) + Cl^- (aq) This three-step mechanism is proposed: NH₃(aq) + OCl^- (aq) Δk1k2 NH₂Cl(aq) + OH- (aq) Fast NH₂Cl(aq) + NH₃(aq) →k3 N₂H₅⁺ (aq) + Cl^- (aq) Slow N₂H₅⁺ (aq) + OH^-(aq) →k4 N₂H₄(aq) + H₂O(l) Fast a. Show that the mechanism sums to the overall reaction.

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Identify the reactants and products in each step of the mechanism.

Write down the reactants and products for each step: Step 1: NH_3(aq) + OCl^-(aq) \rightleftharpoons NH_2Cl(aq) + OH^-(aq), Step 2: NH_2Cl(aq) + NH_3(aq) \rightarrow N_2H_5^+(aq) + Cl^-(aq), Step 3: N_2H_5^+(aq) + OH^-(aq) \rightarrow N_2H_4(aq) + H_2O(l).

Add up all the reactants from each step and all the products from each step.

Cancel out any intermediates or species that appear on both sides of the equation.

Verify that the remaining reactants and products match the overall reaction: 2 NH_3(aq) + OCl^-(aq) \rightarrow N_2H_4(aq) + H_2O(l) + Cl^-(aq).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reaction Mechanism

A reaction mechanism is a step-by-step description of the pathway taken during a chemical reaction. It outlines the individual elementary steps that lead to the overall reaction, including the formation and consumption of intermediates. Understanding the mechanism helps in predicting the rate and outcome of the reaction, as well as identifying the role of catalysts and inhibitors.

Rate-Determining Step

The rate-determining step is the slowest step in a reaction mechanism that controls the overall reaction rate. It is crucial because the speed of this step dictates how quickly the entire reaction proceeds. In the provided mechanism, identifying the slow step allows for a better understanding of how the reaction progresses and how changes in conditions might affect the rate.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced equation. It ensures that the law of conservation of mass is upheld, meaning the number of atoms of each element must be the same on both sides of the equation. In this context, verifying that the sum of the elementary steps matches the overall reaction requires careful stoichiometric analysis.

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How old is a rock that contains 83.2% of the amount of uranium-238 it contained when it was formed?

Textbook Question

Consider the gas-phase reaction: H₂(g) + I₂(g) → 2 HI(g) The reaction was experimentally determined to be first order in H₂ and first order in I₂. Consider the proposed mechanisms. Proposed mechanism I: H₂(g) + I₂(g) → 2 HI(g) Single step Proposed mechanism II: I₂(g) Δk1k-12 I(g) Fast H₂( g) + 2 I( g) → k22 HI( g) Slow a. Show that both of the proposed mechanisms are valid.

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Textbook Question

Consider the gas-phase reaction: H₂(g) + I₂(g) → 2 HI(g) The reaction was experimentally determined to be first order in H₂ and first order in I₂. Consider the proposed mechanisms. Proposed mechanism I: H₂(g) + I₂(g) → 2 HI(g) Single step Proposed mechanism II: I₂(g) Δk1k-12 I(g) Fast H₂( g) + 2 I( g) → k22 HI( g) Slow b. What kind of experimental evidence might lead you to favor mechanism II over mechanism I?

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What rate law corresponds to the proposed mechanism for the formation of hydrogen bromide, which can be written in a simplified form as: Br2(g) → 2Br(g) (Fast) Br(g) + H2(g) → HBr(g) + H(g) (Slow) H(g) + Br2(g) → HBr(g) + Br(g) (Fast)?

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