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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.14 - Chemical Kinetics문제 108a
14장, 문제 108a

Ozone in the upper atmosphere can be destroyed by the following two-step mechanism:
Cl(g) + O3(g) → ClO(g) + O2(g)
ClO(g) + O(g) → Cl(g) + O2(g)
(a) What is the overall equation for this process?

검증된 단계별 안내
1
Identify the reactants and products in each step of the mechanism. In the first step, Cl(g) reacts with O3(g) to form ClO(g) and O2(g). In the second step, ClO(g) reacts with O(g) to regenerate Cl(g) and produce O2(g).
Write down the two given reactions: Step 1: Cl(g) + O3(g) → ClO(g) + O2(g) and Step 2: ClO(g) + O(g) → Cl(g) + O2(g).
Add the two reactions together to find the overall equation. When adding, cancel out any species that appear on both sides of the equation. In this case, ClO(g) and Cl(g) appear on both sides.
After canceling, combine the remaining species to form the overall equation. The reactants are O3(g) and O(g), and the products are O2(g).
Write the overall equation for the process: O3(g) + O(g) → 2O2(g). This represents the net change in the chemical species involved in the mechanism.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
2m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Chemical Reactions

Chemical reactions involve the transformation of reactants into products through the breaking and forming of bonds. In this case, the reactions show how chlorine (Cl) interacts with ozone (O3) to form chlorine monoxide (ClO) and oxygen (O2). Understanding the stoichiometry and conservation of mass is essential for determining the overall reaction.
추천 영상:
가이드 코스
03:31
Chemical Properties

Intermediate Species

In multi-step reactions, intermediate species are formed in one step and consumed in another. Here, ClO is an intermediate that facilitates the regeneration of Cl while also contributing to the destruction of ozone. Recognizing the role of intermediates is crucial for analyzing reaction mechanisms and calculating overall equations.
추천 영상:
가이드 코스
03:03
Amphoteric Species

Overall Reaction Equation

The overall reaction equation summarizes the net change from reactants to products across all steps. To derive it, one must add the individual reactions while canceling out any species that appear on both sides. This process highlights the conservation of atoms and helps in understanding the complete chemical process involved in ozone depletion.
추천 영상:
가이드 코스
07:02
Overall Reaction Equilibrium Constant
관련 실천
교과서 질문

Ozone in the upper atmosphere can be destroyed by the following two-step mechanism:

Cl(g) + O3(g) → ClO(g) + O2(g)

ClO(g) + O(g) → Cl(g) + O2(g) 

(b) What is the catalyst in the reaction?

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교과서 질문

The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.

Step 1: O3(g) ⇌ O2(g) + O(g) (fast)

Step 2: O(g) + O3(g) → 2 O2 (slow)

(b) Derive the rate law that is consistent with this mechanism. (Hint: The product appears in the rate law.)

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교과서 질문

The following mechanism has been proposed for the reaction of NO with H2 to form N2O and H2O:

NO(g) + NO(g) → N2O2(g)

N2O2(g) + H2(g) → N2O(g) + H2O(g)

(d) The observed rate law is rate = k[NO]2[H2]. If the proposed mechanism is correct, what can we conclude about the relative speeds of the first and second reactions?

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교과서 질문

The following mechanism has been proposed for the reaction of NO with H2 to form N2O and H2O:

NO(g) + NO(g) → N2O2(g)

N2O2(g) + H2(g) → N2O(g) + H2O(g)

(a) Show that the elementary reactions of the proposed mechanism add to provide a balanced equation for the reaction.

교과서 질문

The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.

Step 1: O3(g) ⇌ O2(g) + O(g) (fast)

Step 2: O(g) + O3(g) → 2 O2 (slow)

(a) Write the balanced equation for the overall reaction.