2NO(g) + H2(g) --> N2O(g) + H2O(g) + energy.

1. Assume the reaction is reversible and at equilibrium. What shifts in the equilibrium of this reaction are suggested by Le Chateliers Principle?

I think the question should put parameters instead of leaving it so open ended.

Higher T will shift it to the left.
Higher pressure will shift it to the right.
Adding NO or H2 will shift it to the right; adding H2O or N2O will shift it to the left.

Write Kc expressions for the following reactions:

Le Chatelier's Principle states that when a system at equilibrium is subjected to a change in conditions, the system will adjust itself to minimize the effect of that change. In this case, we have the reaction 2NO(g) + H2(g) ↔ N2O(g) + H2O(g) + energy.

Le Chatelier's Principle helps predict how changes in temperature, pressure, and concentration affect the equilibrium of a reaction. Let's consider the different factors one by one:

1. Concentration: If the concentration of any reactant or product is changed, the equilibrium will shift to minimize the effect of the change. For example, if more NO(g) is added, the reaction will shift towards the products (N2O and H2O) to relieve the additional NO(g). On the other hand, if NO(g) is removed, the reaction will shift towards the reactants (2NO and H2) to compensate for the loss.

2. Pressure: Since the number of moles on both sides of the equation is the same (2 mol reactants ↔ 2 mol products), changing the pressure will not have a significant effect on the equilibrium of this reaction.

3. Temperature: The reaction is exothermic (releases energy), and when temperature is changed, the reaction will shift in the direction that absorbs or releases heat to restore equilibrium. If the temperature is increased, the equilibrium will shift towards the reactants (2NO and H2) to consume the excess heat. Conversely, if the temperature is decreased, the equilibrium will shift towards the products (N2O and H2O) to produce more heat.

In summary, Le Chatelier's Principle suggests that the equilibrium of this reaction will shift towards the side with the fewer molecules of gas when concentration is changed, while changes in pressure will have minimal impact. For temperature changes, the reaction will shift in the direction that either absorbs or releases heat.