Consider the reaction H₂(g) + I₂(g) → 2 HI(g). The reaction of a fixed amount of H₂ and I₂ is studied in a cylinder fitted with a movable piston. Indicate the effect of each of the following changes on the rate of the reaction. (c) The addition of a catalyst

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Identify the role of a catalyst in a chemical reaction: A catalyst provides an alternative reaction pathway with a lower activation energy.

Understand that the activation energy is the minimum energy required for a reaction to occur. Lowering this energy increases the number of effective collisions between reactant molecules.

Recognize that by lowering the activation energy, a catalyst increases the rate of the reaction without being consumed in the process.

Note that the presence of a catalyst does not affect the equilibrium position of the reaction; it only helps the system reach equilibrium faster.

Conclude that the addition of a catalyst will increase the rate of the reaction by providing a more efficient pathway for the reaction to proceed.

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Key Concepts

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

Catalysts

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It works by providing an alternative reaction pathway with a lower activation energy, allowing more reactant molecules to collide with sufficient energy to react. This means that even at lower temperatures, reactions can proceed more quickly when a catalyst is present.

Reaction Rate

The reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It can be influenced by several factors, including concentration, temperature, and the presence of a catalyst. Understanding how these factors affect the reaction rate is crucial for predicting how changes in conditions will impact the overall progress of a reaction.

Equilibrium and Dynamic Processes

In a chemical reaction, equilibrium is reached when the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products. The addition of a catalyst does not change the position of equilibrium; it only accelerates the time taken to reach that equilibrium. This concept is essential for understanding how catalysts influence reaction kinetics without altering the final outcome.

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Textbook Question

Consider the reaction H₂(g) + I₂(g) → 2 HI(g). The reaction of a fixed amount of H₂ and I₂ is studied in a cylinder fitted with a movable piston. Indicate the effect of each of the following changes on the rate of the reaction. (a) An increase in temperature at constant volume

Textbook Question

Concentration–time data for the conversion of A and B to D are listed in the following table. (c) What is the rate law?

Textbook Question

Consider the following concentration–time data for the reaction of iodide ion and hypochlorite ion (OCl^-). The products are chloride ion and hypoiodite ion (OI^-).

(a) Write a balanced equation for the reaction.

Consider the reaction H2(g) + I2(g) → 2 HI(g). The reaction of a fixed amount of H2 and I2 is studied in a cylinder fitted with a movable piston. Indicate the effect of each of the following changes on the rate of the reaction. (c) The addition of a catalyst

Verified video answer for a similar problem:

Key Concepts

Catalysts

Reaction Rate

Equilibrium and Dynamic Processes

Consider the reaction H₂(g) + I₂(g) → 2 HI(g). The reaction of a fixed amount of H₂ and I₂ is studied in a cylinder fitted with a movable piston. Indicate the effect of each of the following changes on the rate of the reaction. (c) The addition of a catalyst