Question at position 23 Consider the exothermic formation reaction for ammonia (the Haber process.) Using Le Chatelier's principle, which combinations of external pressure and temperature, T, will drive the reaction to the right to produce more ammonia (NH3) gas? 3H2(g) +N2(g) →2NH3(g)3H_2(g) +N_2(g) →2NH_3(g)Consider the exothermic formation reaction for ammonia (the Haber process.) Using Le Chatelier's principle, which combinations of external pressure and temperature, T, will drive the reaction to the right to produce more ammonia (NH3) gas? 3H2(g) +N2(g) →2NH3(g)3H_2(g) +N_2(g) →2NH_3(g)high T and low P high T and high P low T and low P low T and high P

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BlackTom AI · Accepted Answer

When applying Le Chatelier's principle to the Haber process, we must consider both temperature and pressure effects on the exothermic gas-phase reaction: 3H2(g) + N2(g) → 2NH3(g).

First, assess temperature effects: the reaction is exothermic, which means it releases heat. Increasing temperature drives the equilibrium toward the reactants (endothermic direction) to absorb the added heat, while decreasing temperature shifts toward the products to release heat. In other words, lower temperatures favor NH3 formation, higher temperatures oppose it.

Next, assess pressure effects: the total number of gas moles on each side is 4 moles of reactants and 2 moles of product. Increasing external pressure shifts the equilibrium toward the side with fewer gas moles, which is the product side (NH3). Conversely, lowering pressure shifts toward the side with more gas moles (the reactants).

Now evaluate each option:
- High T and low P: High temperature disfavors NH3 formation (drives to reactants), and low pressure provides less incentive to form the fewer-molecule product side. This combo is clearly not favorable for producing more NH3.
- High T and high P: While high pressure helps push toward fewer gas moles, the simultaneous high temperature shifts equilibrium away from NH3 due to the exothermic nature. So the net effect is still not optimal for maximizing NH3.
- Low T and low P: Low temperature helps NH3 formation, but low pressure reduces the driving force toward the product side, since pressure benefit is weaker when pressure is not elevated. This reduces the overall drive to NH3 compared with a high-pressure scenario.
- Low T and high P: This combination simultaneously exploits both favorable effects: low temperature promotes formation of NH3 (exothermic direction), and high pressure favors the side with fewer gas moles (NH3). Therefore, this scenario most effectively drives the reaction to the right and increases NH3 yield.

In summary, the most effective conditions to push the Haber process toward more NH3 are those with low temperature and high pressure, which aligns with Le Chatelier's principle for this exothermic, gas-phase reaction.

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