An equilibrium constant (K) with a value of 1.5x10-9 indicates that at equilibrium: the reaction is product-favored. the reaction is reactant-favored. approximately equal concentrations of reactants and products are present. there are more products present than reactants.

What is the correct equilibrium constant expression for the balanced reaction shown below? 2 HCl (g) + I2 (s)   2 HI (g) + Cl2 (g)

Given the following equation: NH4 (aq) + NO2 (aq) → N2(g) + 2H2O (1) AH = -122.4 kJ/mol How would decreasing the pressure effect the equilibrium? It would cause the equilibrium to shift to the right, favoring the products or the forward reaction. It would cause the equilibrium to shift to the left, favoring the reactants or the reverse reaction. It would not effect the equilibrium.

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) A catalyst is added to the reaction mixture. which will happen? the equilibrium will not shift  the equilibrium will shift towards product but keq will not change the equilibrium will shift towards reactant but keq will not change     the equilibrium will shift towards product and keq will increase the equilibrium will shift towards reactant and keq will decrease (b) The total pressure of the system is increased by adding a noble gas.       (c) Cl2(g) is removed from the system.

Please don't provide handwritten solution ....

Indicate whether or not product formation increases if the size of the reaction container is decreased for each of the following equilibrium systems. a) 4NH3(g) + 5O2(g)  heat + 4NO(g) + 6H2O(g)                                b) heat + 2NaHCO3(s)   Na2CO3(s) + CO2(g) + H2O(g)

Most reaction do not go to completions. Equilibrium is established between the reactants and products. For the reaction of A with B to produce C and D, we can write the chemical equation as: аА + bв + сс + dD where + represents equilibrium between the reactants and products. The extent to which the reaction proceeds to product formation, at a given temperature, is given by the equilibrium constant, Kę. The equilibrium constant is written mathematically (for the above equation) as: [C[[D]* K. = [A]°[B]" where, a, b, c, and d are the stoichiometric coefficients from the balanced chemical equation and the brackets, [ ], indicate molar concentration. 1. For the following reaction: 2A + В + 3с calculate the equilibrium constant, K, if at equilibrium the concentration of A is 0.15M, the concentration of B is 0.20M, and the concentration of C is 0.10M.

Please answer number 1

Write the equilibrium-constant expression for the reaction shown in terms of [SO2], [CO2], [CS2], and [O2]. 2SO2(g)+CO2(g)↽−−⇀CS2(g)+3O2(g) ?c, which is sometimes symbolized as ? or ?eq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, ?c means the same thing as ? and ?eq.