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
To increase the yield of NH3 in the reaction N2(g) + 3H2(g) <=> 2NH3(g), you can make certain changes that will shift the equilibrium towards the formation of more NH3. Let's analyze each option and explain how it affects the equilibrium:
(a) ▲[N2]: Increasing the concentration of N2 will shift the equilibrium towards the right side of the reaction, according to Le Chatelier's principle. This means that more NH3 will be produced. To increase the concentration, you can add more N2(g) to the reaction vessel.
(b) ▲T of the chamber storing NH3: Changing the temperature of the chamber where NH3 is stored does not directly impact the yield of NH3. However, it can affect the equilibrium position. According to Le Chatelier's principle, increasing the temperature favors the endothermic reaction (the forward reaction in this case) to absorb the excess heat. So, if you increase the temperature, the equilibrium will shift to the right, resulting in more NH3 being produced.
(c) ▲P of the system: Changing the pressure of the system will also impact the equilibrium position. In this case, increasing the pressure will favor the side with fewer moles of gas. The reaction has a total of 4 moles of gas on the left side (N2 and H2) and 2 moles of gas on the right side (NH3). Therefore, increasing the pressure will shift the equilibrium to the right and increase the yield of NH3.
(d) ▲[NH3(g)]: Increasing the concentration of NH3 will not directly affect the equilibrium position. According to Le Chatelier's principle, increasing the concentration of a product will cause the reaction to shift in the opposite direction. Consequently, increasing the concentration of NH3 will shift the equilibrium to the left, resulting in less NH3 being produced.
In summary, options (a), (b), and (c) will increase the yield of NH3, while option (d) will have the opposite effect.