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
I'm a little confused by the question; I may write more than is necessary. This question is about Le Chatelier's principle and which direction the reaction will shift. Shift to the right means more NH3 is produced at the expense of N2 and H2. Shift to the left means NH3 is decreasing while N2 and H2 are increasing.
Adding N2 or H2 shifts to the right. Removing N2 or H2 shifts to the left.
Increasing T of NH3 shifts to the left. Decreasing T of NH3 shifts to the right.
Delta P of the system--increase P shifts to the right; decreasing P shifts to the left.
Add NH3 shift to the left; remove NH3 shifts to the right.
To understand how each factor influences the yield of NH3, let's consider the reaction in more detail. The reaction you have shown is the formation of ammonia (NH3) from nitrogen gas (N2) and hydrogen gas (H2). The reaction is an equilibrium reaction, meaning it can proceed in both the forward and reverse directions.
The reaction can be represented as follows:
N2(g) + 3H2(g) <=> 2NH3(g) + ΔH
(a) Δ[N2]: Changing the concentration of N2 affects the position of equilibrium and, consequently, the yield of NH3. According to Le Chatelier's principle, increasing the concentration of N2 will shift the equilibrium towards the reactant side (N2 and H2) to counteract the disturbance. As a result, the yield of NH3 will decrease.
(b) ΔT of the chamber storing NH3: Changing the temperature has a significant impact on the equilibrium position. In this case, increasing the temperature will favor the endothermic reaction (the forward reaction), which absorbs heat. As a result, the equilibrium will shift in the forward direction, leading to an increase in the yield of NH3.
(c) ΔP of the system: Changing the pressure can influence the equilibrium position if the number of moles of gas changes. In this reaction, there are four moles of gas on the left side (N2 and H2) and two moles of gas on the right side (NH3). According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas. Therefore, the equilibrium will shift towards the reactant side, decreasing the yield of NH3.
(d) Δ[NH3(g)]: Changing the concentration of NH3 does not directly affect the equilibrium position since it is a product in this reaction. However, removing NH3 as it forms can shift the equilibrium forward to counteract its removal. This means that decreasing the concentration of NH3 (removing it from the system) will lead to an increase in the yield of NH3.
In summary, increasing the temperature (b) and decreasing the concentration of NH3 (d) will increase the yield of NH3. Conversely, increasing the concentration of N2 (a) and the pressure (c) will decrease the yield of NH3.