Consider the chemical equation below. 2 NO2(g) equilibrium reaction arrow N2O4(g
ID: 939425 • Letter: C
Question
Consider the chemical equation below. 2 NO2(g) equilibrium reaction arrow N2O4(g) The equilibrium constant for this chemical reaction at a certain temperature and pressure is Kc = 0.51. Determine if the reaction favors the products, reactants, or neither. Step 1 of 2 Write the expression for the equilibrium constant for the reaction. When equilibrium is attained in a reversible reaction, the ratio of the molar concentrations of the products to that of the reactants is defined as equilibrium constant (Kc). In the given reaction, the equilibrium constant expression is the following. (Concentration equilibrium expressions take the general form: Kc = [HCl]2 / [H2] . [Cl2]. Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPadHelp Each reactant and product is raised to its coefficients from the balanced equation for the reaction. Given a chemical reaction at heterogeneous equilibrium, write the equilibrium-constant expression for the reaction in terms of concentrations of the components that are not pure solids, pure liquids, or the solvent. Step 2 of 2 Evaluate the equilibrium-constant expression to determine how the magnitude of the equilibrium constant is related to the equilibrium position. If Kc > 1, the numerator is than the denominator. Therefore, the equilibrium concentration of the is greater than the concentration of the , and the reaction favors the . If Kc < 1, the numerator is than the denominator. Therefore, the equilibrium concentration of the is greater than the concentration of the , and the reaction favors the . If Kc = 1, the numerator and denominator are . Therefore, the equilibrium concentrations of reactants and products are , and the reaction favors neither the reactants nor the products. Because Kc for the given equation (0.51) is , the equilibrium for the given reaction must lie to the , with the .
Explanation / Answer
2 NO2 <--------------------> N2O4
expression for the equilibrium constant for the reaction : Kc =[N2O4]/[NO2]^2
Kc = 0.51
Kc < 1. reaction favours to reactant side.