Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (K) [H2] [NH3] [KC] [N2] 500 0.115 0.105 0.439 575 0.110 M - 0.124 M 9.6 775 0.125 M 0.140 M 0.0584

12.102 A chemical engineer is working to optimize the production of acrylonitrile to be used in the manufacture of carbon fibers. The reaction being used is the combination of propene gas, ammonia, and oxygen. The reaction is normally carried out at moderately high temperatures so all species are in the gas phase. (a) Write the equilibrium constant expression for this reaction. (b) The boiling point of acrylonitrile is 77 °C, and that of propene is -48 °C. What would the equilibrium expression be if this reaction were carried out at room temperature? (c) What characteristic of this reaction might cause the engineer to desire carrying out this reaction at room temperature?

In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.

What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.