Determine the equilibrium constant KP for the reaction CH4+2 O2 ⇌CO2+2 H2 O at 25^∘ C.

Name: Problem 23, Chapter 16: Thermodynamics: An Engineering Approach
Uploaded: 2020-11-03T03:09:41-08:00
Duration: 3 min 32 s
Channel: Rory Naguib
Description: Determine the equilibrium constant KP for the reaction CH4+2 O2 ⇌CO2+2 H2 O at 25^∘ C.

step 1 Problem number 22. First, the KIPS function of the reaction is determined from the KIP's functio

Determine the equilibrium constant KP for the reaction CH4+2...

Key Concepts

Equilibrium Constant (K?)

The equilibrium constant expressed as K? for gaseous reactions is defined in terms of the partial pressures of the reactants and products. It is calculated by taking the ratio of the product of the partial pressures of the products to that of the reactants, with each partial pressure raised to the power of its stoichiometric coefficient. K? provides a quantitative measure of the position of equilibrium in a gas-phase reaction.

Reaction Stoichiometry

Reaction stoichiometry refers to the balance of reactants and products in a chemical equation, which is essential when writing the equilibrium expression. The stoichiometric coefficients from the balanced equation indicate the exponents to which the partial pressures or concentrations are raised in the equilibrium constant expression, ensuring the relationship accurately reflects the reaction's progress.

Chemical Equilibrium

Chemical equilibrium is the state in a reversible reaction when the rate of the forward reaction equals the rate of the reverse reaction, meaning that the concentrations or partial pressures of reactants and products remain constant over time. This concept underpins the analysis of reactions as it explains how systems settle into a stable composition under fixed conditions.

Temperature Dependence

The equilibrium constant is dependent on temperature; changes in temperature can alter the value of K?. At a given temperature, typically expressed in Kelvin, K? can be related to the standard Gibbs free energy change (?G°) of the reaction. This relationship, often represented as K = exp(-?G°/RT), shows how thermodynamic properties govern the position of equilibrium.

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