Chemical Equilibrium and Stoichiometry

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Questions and Answers

What is the primary criterion for a reaction to be at equilibrium?

The concentration of products exceeds that of reactants.

The forward and reverse reaction rates are equal. (correct)

The reaction has gone to completion.

The concentrations of reactants and products are equal.

What is represented by the terms in an ICE table?

Intermediate concentrations, Change, Equilibrium temperatures

Intermittent concentrations, Cumulative change, Equilibrium times

Initial concentrations, Change in concentrations, Equilibrium concentrations (correct)

Initial concentrations, Change in concentrations, Energy released

How is the equilibrium constant (Kc) calculated?

By finding the product of initial concentrations only.

By multiplying products' concentrations and dividing by reactants' concentrations. (correct)

By taking the sum of products' concentrations minus reactants' concentrations.

By averaging the concentrations of all reactants and products.

What does a large value of Kc indicate about a reaction?

The reaction favors the formation of products. Signup and view all the answers

What is the function of the reaction quotient (Q)?

Q assesses the relative amounts of reactants and products at any moment. Signup and view all the answers

If Q > Kc, what will the reaction do?

Shift to the left to produce more reactants. Signup and view all the answers

When using an ICE table, what does the variable 'x' represent?

The change in concentration from initial to equilibrium. Signup and view all the answers

What should be done if the Kc expression is complex during calculations?

Identify values and apply the quadratic formula. Signup and view all the answers

What occurs in a chemical reaction at dynamic equilibrium?

The concentrations of reactants and products remain constant. Signup and view all the answers

Which statement best describes stoichiometry in relation to equilibrium reactions?

Stoichiometry does not account for changes in equilibrium conditions. Signup and view all the answers

Why are ICE tables useful in studying chemical equilibrium?

They show both the changes and the final equilibrium concentrations. Signup and view all the answers

What is indicated by a small value of the equilibrium constant, Kc?

The reactants are favored at equilibrium. Signup and view all the answers

When Kc >> 1, what can be inferred about the reaction?

The products are favored at equilibrium. Signup and view all the answers

What do initial concentrations in an ICE table represent?

The concentrations of reactants before any change occurs. Signup and view all the answers

How is the relationship between reactants and products affected at equilibrium?

The ratio of products to reactants always equals Kc. Signup and view all the answers

Study Notes

Chemical Equilibrium

Chemical reactions can be reversible, with reactants forming products and products reforming reactants.
Dynamic equilibrium occurs when the rates of the forward and reverse reactions are equal. The reaction appears to stop, but both forward and reverse reactions continue at equal rates.
Equilibrium results in constant concentrations of reactants and products despite ongoing chemical activity.

Stoichiometry

Stoichiometry predicts the limiting reactant and product yield, assuming a reaction goes to completion.
Equilibrium reactions are more complex as product formation is affected by equilibrium conditions.

ICE Tables

ICE tables (Initial, Change, Equilibrium) are used for calculating equilibrium concentrations.

Equilibrium Constant (Kc)

Kc is the equilibrium constant for a reaction, calculated as the ratio of product concentrations (raised to their stoichiometric coefficients) to reactant concentrations (raised to their stoichiometric coefficients).
Kc is a measure of the relative amounts of reactants and products at equilibrium.
A large Kc (Kc >> 1) favors product formation at equilibrium.
A small Kc (<1) favors reactant formation at equilibrium.

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Description

This quiz covers the fundamental concepts of chemical equilibrium, including the forward and reverse reactions and the use of the ICE table for equilibrium calculations. Understanding the equilibrium constant (Kc) is also highlighted, along with practical example calculations. Test your knowledge and skills in chemical reaction dynamics.