The following pictures represent the initial and equilibrium states for the exothermic reaction of solid A (red) with gas- eous B2 (blue) to give gaseous AB. (a) Write a balanced chemical equation for the reaction.

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Identify the reactants and products from the description: solid A and gaseous B2 react to form gaseous AB.

Write the unbalanced chemical equation: A (solid) + B2 (gas) -> AB (gas).

Balance the equation by ensuring the number of atoms of each element is the same on both sides.

Since B2 is a diatomic molecule, you may need to adjust coefficients to balance the B atoms.

Check the balance of the equation: ensure the number of A and B atoms are equal on both sides.

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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 during the reaction. Balancing involves adjusting coefficients in front of the chemical formulas to achieve this equality.

Exothermic Reaction

An exothermic reaction is a type of chemical reaction that releases energy, usually in the form of heat, to its surroundings. This occurs when the total energy of the products is lower than that of the reactants, resulting in a net release of energy. Understanding this concept is crucial for predicting temperature changes and the direction of the reaction.

States of Matter

The states of matter refer to the distinct forms that different phases of matter take on, primarily solid, liquid, and gas. In the context of chemical reactions, the state of each reactant and product can influence reaction rates and equilibrium. Recognizing the states of matter involved helps in writing accurate chemical equations and understanding the behavior of substances during reactions.

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Textbook Question

The following picture represents the equilibrium state for the reaction 2 AB ∆ A2 + B2. Which rate constant is larger, kf or kr? Explain.

Textbook Question

The following pictures represent the initial and equilibrium states for the exothermic decomposition of gaseous A mol- ecules (red) to give gaseous B molecules (blue).(b) Will the number of A molecules in the equilibrium mix- ture increase, decrease, or remain the same after each of the following changes? Explain.(3) Increasing the pressure by adding an inert gas

Textbook Question

The following pictures represent the initial and equilibrium states for the exothermic decomposition of gaseous A mol- ecules (red) to give gaseous B molecules (blue). (a) Write a balanced chemical equation for the reaction.

Textbook Question

Identify the true statement about the rate of the forward and reverse reaction once a reaction has reached equilibrium. (a) The rate of the forward reaction and the reverse reaction is zero. (b) The rate of the forward reaction is greater than the rate of the reverse reaction. (c) The rate of the reverse reaction is greater than the rate of the forward reaction. (d) The rate of the forward reaction is equal to the rate of the reverse reaction.