At 100 °C, Kc = 4.72 for the reaction 2 NO21g2 ∆ N2O41g2. An empty 10.0-L flask is filled with 4.60 g of NO2 at 100 °C. What is the total pressure in the flask at equilibrium?

The equilibrium constant, Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2 NO2(g) ⇌ N2O4(g), Kc = [N2O4]/[NO2]^2. A Kc value greater than 1 indicates that at equilibrium, products are favored over reactants.

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the total pressure in a gas system, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In the context of gaseous reactions, it helps determine the moles of gases involved at equilibrium, which is crucial for calculating total pressure. Understanding the stoichiometric coefficients allows for the correct application of Kc to find equilibrium concentrations.