Given the reaction NH3(g) + O2(g)--> NO(g) + energy, in what direction will the reaction shift if you:

a)remove O2 (g)
b)increase the pressure by decreasing the volume
c)decrease the temperature
d)add a catalyst

I have re-written the equation as

NH3(g) + O2(g)--> NO(g) + heat

Le Chatelier's Principle says that a system will try to undo what we do to it. Therefore, if we add heat, for example, the system will try to get rid of the extra heat. How can it do that? By shifting to the left (reacting in the reverse direction) because that way some of the added heat will be used up.
The others are done the same way. Someone will be happy to check your answers.

To determine the direction in which the given reaction will shift in each scenario, we need to consider Le Chatelier's Principle. Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in conditions, the equilibrium will adjust to counteract the change and establish a new equilibrium.

a) If O2 (g) is removed, the reaction will shift towards the side with fewer moles of gas. In this case, the right side of the equation has fewer moles of gas (1 mole) compared to the left side (2 moles). Therefore, the reaction will shift to the right, producing more NO (g).

b) If the pressure is increased by decreasing the volume, the reaction will shift towards the side with fewer moles of gas. Again, the right side of the equation has fewer moles of gas (1 mole) compared to the left side (2 moles). Hence, the reaction will shift to the right, favoring the formation of more NO (g).

c) When the temperature is decreased, the reaction will shift towards the side that produces heat. As the given reaction is exothermic (energy is released), lowering the temperature will favor the backward reaction to produce more NH3 (g) and O2 (g).

d) Adding a catalyst does not shift the equilibrium position of a reaction. Instead, it increases the rate of both the forward and backward reactions equally, allowing the system to reach equilibrium faster but with the same composition.

In summary:
a) Removing O2 (g) shifts the reaction to the right.
b) Decreasing the volume increases the pressure, favoring the reaction to the right.
c) Decreasing the temperature favors the backward reaction.
d) Adding a catalyst does not shift the equilibrium position.