N2(g)+3H2(g)<=>2NH3(g) +▲H

if uou are preparing NH3, hiw does the following increase the yield of NH3?
(a) ▲[N2] ▲[H2]
(b) ▲T of the chamber storing NH3
(c) ▲P of the system
(d) ▲[NH3(g)]

* <=> equilibrium
* ▲ change

If you increase the N2 or H2 concentrations that is going to force the production of NH3

If you increase the temperature, to maintain equilibrium heat has to be given off. Which means more NH3

If you add pressure you need fewer molecules which again causes the production of NH3 ( you have 2 molecules there vs. 5 molecules on the other side)

If you remove NH3 then more NH3 will be produced.

To understand how each factor affects the yield of NH3 in the given reaction, let's go through them one by one:

(a) ▲[N2]: Increasing the concentration of N2 (i.e., increasing [N2]) will shift the equilibrium towards the products to balance the change. In this case, it will favor the formation of NH3 to counteract the increase in N2 concentration. As a result, the yield of NH3 will increase.

(b) ▲T of the chamber storing NH3: Changing the temperature of the system will affect the equilibrium position based on the reaction's enthalpy, ▲H. In this case, the reaction is exothermic (▲H < 0) since heat is released in the forward reaction (formation of NH3). According to Le Chatelier's principle, increasing the temperature for an exothermic reaction will shift the equilibrium in the reverse direction to consume the excess heat. Hence, increasing the temperature will decrease the yield of NH3.

(c) ▲P of the system: Changing the pressure of the system will have an effect if the number of moles of gas differs between the reactants and products. In this case, there is a difference since there are fewer moles of gas on the product side (2 moles of NH3) compared to the reactant side (3 moles of H2). According to Le Chatelier's principle, increasing the pressure will favor the formation of fewer moles of gas. Therefore, increasing the pressure will shift the equilibrium towards the product side, increasing the yield of NH3.

(d) ▲[NH3(g)]: Changing the concentration of NH3 will not directly affect the equilibrium position because it appears in the balanced equation with a coefficient of 2. However, if you were to remove some NH3 from the system, for example, the equilibrium will shift towards the reactants to replenish the lost NH3. This will increase the yield of NH3 until reaching a new equilibrium.

In summary:
- Increasing [N2] and ▲P of the system will increase the yield of NH3.
- Increasing ▲T of the chamber storing NH3 will decrease the yield of NH3.
- ▲[NH3(g)] will not directly affect the equilibrium position but can be used to manipulate the system to increase the yield of NH3 by removing some of it.

Remember, these explanations apply to the given reaction and are based on Le Chatelier's principle. The actual effect may vary depending on other factors and the specific conditions of the reaction.