Use your answer from Problem 7.54 to calculate the following:[O2] at equilibrium when [CO2] = 0.18 mol/L and [CO] = 0.0200 mol/L

Verified step by step guidance

1. Identify the chemical reaction involved and write the balanced equation. For example, if the reaction is CO + 1/2 O2 -> CO2, ensure it is balanced.
2. Use the equilibrium constant expression for the reaction. For the example reaction, the expression is Kc = [CO2]/([CO][O2]^(1/2)).
3. Substitute the given concentrations into the equilibrium expression. Here, [CO2] = 0.18 mol/L and [CO] = 0.0200 mol/L.
4. Rearrange the equilibrium expression to solve for the unknown concentration, [O2].
5. Calculate the value of [O2] using the rearranged expression and the known values.

Key Concepts

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It is specific to a particular reaction at a certain temperature. Understanding K helps predict the direction of the reaction and the concentrations of reactants and products at equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle is crucial for predicting how changes in concentration, pressure, or temperature will affect the concentrations of reactants and products in a chemical reaction.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows for the determination of the relationships between the amounts of substances consumed and produced. In this context, stoichiometry is essential for calculating the concentration of O2 at equilibrium based on the given concentrations of CO2 and CO.