24. The most probable molecular energy (kT) at 27°C is. • What fraction of the Rubidium Fluoride ion pairs have enough kinetic energy to dissociate in the gas phase? • What fraction of the Rubidium Fluoride ion pairs have enough kinetic energy to dissociate in the aqueous solution?

The equilibrium constant changes when...   a a catalyst is added. b the temperature changes. c the surface area changes. d the concentration of reactants changes e more than one above is correct

If the equilibrium constant for a reaction is very large, what is the reaction

When solid lead(II) phosphate is in equilibrium with its ions, the ratio of lead(II) ions to phosphate ions is which of the following? 2:1 3:2 1:1 2:3 1:2

Use Le Châtelier’s Principle to explain the effect each of the following changes will have upon the system—will the equilibrium shift toward the product or reactant side? Why? N2(g) + 3 H2(g)  ↔ 2 NH3(g) + heat a. If more hydrogen is added to the system the equilibrium will shift to the..... (pick one and explain)i. Right ii. Left iii. Remains unchanged b. If ammonia is removed from the system the equilibrium will shift to the..... (pick one and explain)i. Right ii. Left iii. Remains unchanged c. If nitrogen is removed from the system the equilibrium will shift to the..... (pick one and explain)

4. Which of the following statements is false? A. Increasing the volume of the container will couse the reaction to shift to the left. B. Decreasing the volume of the container will cause the partial pressure of N2 to increase. C. Adding an inert gas such as Neon will couse the pressure in the container to increase. D. Decreasing the partial pressure of NO will cause the partial pressure of N2 to increase. E. The addition of a catalyst will speed up the reaction but will have no effect on the position of equilibrium.