11. Since the formation of water from its elements is highly spontaneous, how is it possible to collect the product gases as described in Question 10? Is the mixture of and gases at equilibrium? How can they be made to come to equilibrium again, and what would be the resulting substance?

12. If the gases obtained as described in Question 10 are collected in a tank that then is sealed, and if the tank has a total interior pressure of 0.5 atm, what is the partial pressure of each gas?

13. Which reaction is more spontaneous, starting from standard conditions, the synthesis of HCl, , or ? In which reaction will more of the starting materials remain unreacted when equilibrium has been reached?

14. What is the difference between , , and ? What is the relationship between and for the ammonia synthesis reaction when written as + ?

15. What is the general expression relating and for gases?

16. Dalton's law of partial pressures tells us that partial pressure is related to mole fraction in a gas mixture by the expression
p = P , in which P is the total pressure. What is the general expression relating and for gases?

17. What is Le Chatelier's principle? What would it indicate about the effect on an equilibrium constant of raising the temperature at which the reaction took place?

18. How can Le Chatelier's principle predict the effect on equilibrium concentrations of a change in overall pressure?

19. Does a change in pressure bring about a change in the numerical value of the equilibrium constant, ? Does a change in temperature lead to a change in numerical value of ?

20. If a reaction has a large negative standard free energy change, is the reaction spontaneous if started from standard conditions? What is meant by standard conditions? Will the equilibrium constant for this reaction be large, or small, and how is it related to the standard free energy change?