A system, which contains only molecules as reactantsand products, is at equilibrium. Describe what happensto the concentrations of the reactants and products andwhat happens to individual reactant and productmolecules.

Which of the following may change the ratio of products to reactants in an equilibrium mixture for a chemical reaction involving gaseous species?           1. Increasing the temperature.               2. Adding a catalyst              3. Adding gaseous reactants

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 75.0L tank with 6.5 mol of sulfur dioxide gas and 29.mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 3.3 mol.Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits

The reaction of NOCI(g) + CI(g) → NO(g) + Cl2(g) is found to have an equilibrium constant of 9.1x10-9 at a particular temperature. What does this mean? Periodic Table and Datasheet O At equilibrium, there is a much higher concentration of reactants than products. O At equilibrium, there is a much higher concentration of products than reactants. At equilibrium, there is an equal concentration of reactants and products. At equilibrium, the value of the equilibrium constant depends on the initial concentration(s).