The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism. Step 1: O 3 (g) ⇌ O 2 (g) + O(g) (fast) Step 2: O(g) + O 3 (g) → 2 O 2 (slow) (a) Write the balanced equation for the overall reaction.

Hello. In this problem, we are asked to provide the balanced chemical equation for the overall reaction of the following mechanism. So to come up with the balanced equation we need to cancel things that appear on opposite sides. So we see that we have sulfur trioxide on the product side and then on the reactant side on the product side it has two moles of sulfur trioxide, and on the reactant side it only has one. So in order to get them to balance, we need to have a coefficient of two in front of both of them. So we are going to multiply this second reaction, everything by two. So let's write our reactions out then. So we'll have to sulfur dioxide because oxygen Goes to two moles of sulfur trioxide and the multiplying the next equation, everything by two, we get two moles of sulfur trioxide Plus two moles of water, supposed to form two moles of sulfuric acid. And so now our two moles of sulfur trioxide will cancel. And now we combine everything that appears on the reactive side together and then everything that appears on the product side together. So we get two moles of S. 02 dioxide gas plus oxygen Plus two moles of water Goes to form two moles of sulfuric acid. And so at this point in time it's also a good idea to go back through and double check this equation to ensure that everything is indeed balanced. Thanks for watching. Hope this helps

Ch.14 - Chemical Kinetics

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Brown 15th Edition

Ch.14 - Chemical Kinetics

Problem 109a

Chapter 14, Problem 109a

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.

Verified step by step guidance

Identify the reactants and products in each step of the mechanism. In Step 1, ozone (O3) decomposes into oxygen (O2) and an oxygen atom (O). In Step 2, the oxygen atom (O) reacts with another ozone molecule (O3) to form two oxygen molecules (2 O2).

Add the two steps together to find the overall reaction. This involves summing up all reactants and products from both steps.

Cancel out any intermediates that appear on both sides of the reaction. In this case, the oxygen atom (O) is an intermediate that appears as a product in Step 1 and a reactant in Step 2, so it cancels out.

Combine the remaining reactants and products to write the balanced equation for the overall reaction. After canceling the intermediate, you should have the reactants and products that represent the overall process.

Verify that the equation is balanced by ensuring that the number of each type of atom is the same on both sides of the equation. This confirms that the overall reaction is correctly represented.

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Key Concepts

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

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. This ensures the law of conservation of mass is upheld, meaning that matter is neither created nor destroyed in a chemical reaction. Balancing involves adjusting coefficients in front of the chemical formulas to achieve this equality.

Reaction Mechanism

A reaction mechanism is a detailed description of the steps involved in a chemical reaction, including the sequence of elementary reactions. Each step can vary in speed, with some being fast and others slow, which affects the overall rate of the reaction. Understanding the mechanism helps in predicting the products and the rate of the reaction.

Elementary Reactions

Elementary reactions are single-step processes that describe the direct transformation of reactants into products. Each elementary reaction has its own rate law, which can be determined experimentally. In the given mechanism, the first step is fast and reversible, while the second step is slow and irreversible, influencing the overall reaction dynamics.

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Related Practice

Textbook Question

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?

Textbook Question

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?

Textbook Question

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?

Textbook Question

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.)

Textbook Question

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)

(d) If instead the reaction occurred in a single step, would the rate law change? If so, what would it be?

Textbook Question

The following mechanism has been proposed for the gasphase reaction of chloroform 1CHCl32 and chlorine:

Step 1: Cl₂(g) k₁⇌ k_-1 2 Cl(g) (fast)

Step 2: Cl(g) + CHCl₃(g) k₂→ HCl(g) + CCl₃(g) (slow)

Step 3: Cl(g0 + CCl3(g) k₃→ CCl₄ (fast)

(e) What is the rate law predicted by this mechanism? (Hint: The overall reaction order is not an integer.)

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.

Verified video answer for a similar problem:

Key Concepts

Balanced Chemical Equation

Reaction Mechanism

Elementary Reactions

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.