Predict how changes effects equilibrium for N2(g) + 3H2(g) -----> 2NH3(g) + heat

a. add heat
b. remove heat
c. add NH3(g)
d. remove NH3(g)

Le Chatelier's Principle says, in ordinary terms, that a system in equilibrium tries to undo what we do to it.

a. This system produces heat. Therefore, if we ADD heat to it it must try to get rid of it. How can it do that? Simple. By shifting to the left it USES heat and that's how it gets rid of what we've added.
With that you should be able to do the others.

Does that mean when heat is added it favors the reactant side?

To predict how changes will affect the equilibrium for the given reaction, we need to apply Le Chatelier's principle. Le Chatelier's principle states that if a system at equilibrium is subjected to a change in conditions, the system will react in such a way as to counteract the change and restore equilibrium.

a. Add heat:
When heat is added to the system, the reaction shifts in the endothermic direction to absorb the excess heat. In this case, the reaction would shift to the right, producing more NH3 (g).

b. Remove heat:
When heat is removed from the system, the reaction shifts in the exothermic direction to release more heat. To counteract the heat removal, the reaction would shift to the left, producing more N2 (g) and H2 (g).

c. Add NH3 (g):
Adding NH3 (g) to the system would increase the concentration of the product, which disrupts the equilibrium. In response, the reaction would shift to the left to consume some of the additional NH3 (g) and restore equilibrium.

d. Remove NH3 (g):
Removing NH3 (g) from the system would decrease the concentration of the product, causing the reaction to shift to the right to produce more NH3 (g) and restore equilibrium.

So, the effects on equilibrium are as follows:
a. Add heat: Shifts the equilibrium to the right, producing more NH3 (g).
b. Remove heat: Shifts the equilibrium to the left, producing more N2 (g) and H2 (g).
c. Add NH3 (g): Shifts the equilibrium to the left, reducing the concentration of NH3 (g).
d. Remove NH3 (g): Shifts the equilibrium to the right, producing more NH3 (g).

To predict how changes will affect the equilibrium of a chemical reaction, we need to consider Le Chatelier's principle. According to this principle, when a system at equilibrium is subjected to a change, it will shift in a way that minimizes the effect of that change. Let's analyze the given changes and their effect on the equilibrium:

a. Adding Heat: In the given reaction, heat is already a product. When heat is added, the reaction will shift in the reverse direction to consume the excess heat. It will favor the reactants (N2 and H2) and form more reactants, thereby decreasing the concentration of NH3.

b. Removing Heat: Removing heat will cause the system to shift in the forward direction to replace the lost heat. It will favor the products (NH3) and form more products, increasing the concentration of NH3.

c. Adding NH3: Adding NH3, which is one of the products, will cause the system to shift in the reverse direction to consume the excess NH3. It will favor the reactants (N2 and H2), resulting in a decrease in NH3 concentration.

d. Removing NH3: Removing NH3 will cause the system to shift in the forward direction to replace the lost NH3. It will favor the products (NH3), leading to an increase in NH3 concentration.

Based on Le Chatelier's principle, we can conclude:

a. Adding heat will shift the reaction to favor the reactants and decrease NH3 concentration.
b. Removing heat will shift the reaction to favor the products and increase NH3 concentration.
c. Adding NH3 will shift the reaction to favor the reactants and decrease NH3 concentration.
d. Removing NH3 will shift the reaction to favor the products and increase NH3 concentration.