The equilibrium system between sulfur dioxide gas, oxygen gas, and sulfur trioxide gas is given. 2 SO₂(g) + O₂(g) 2 SO3(g) Write the balanced chemical equation for the reverse reaction. Include physical states for all species.

Consider the following system at equilibrium: CH4(g)  +  H2O(g) D CO (g) + 3H2 (g)     ΔH° = +206 kJ.      Which of the following changes will shift the equilibrium to the left?    decreasing the pressure     adding a catalyst     adding methane     increasing the temperature     decreasing the volume

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

Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium? A system has reached equilibrium when the concentrations of reactants and products remain constant. A system has reached equilibrium when the reaction has stopped and no more products are formed. A system has reached equilibrium when the rate constant for the forward reaction equals the rate constant of the reverse reaction. A system has reached equilibrium when the concentrations of reactants and products correspond to the stoichiometric ratios determined by the balanced equation.

The equilibrium system between hydrogen gas, bromine gas, and hydrogen bromide gas is given. H, (g) + Br, (g) = 2 HBr(g) Write the balanced chemical equation for the reverse reaction. Include physical states for all species. chemical equation:

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.

Suppose a 250. mL flask is filled with 1.6 mol of I, and 1.3 mol of HI. This reaction becomes possible: H,(g) +I,(g) = -2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H,. You can leave out the M symbol for molarity. H, I, HI initial change equilibrium olo X

Consider the reaction: 2 CO(g) + O2(g)=2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.