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)low T and high Plow T and low P high T and high P high T and low P

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BlackTom AI · Accepted Answer

The question asks which combination of external pressure and temperature will drive the Haber process to the right, increasing NH3 production.
First, restating the options helps: Option A: low T and high P; Option B: low T and low P; Option C: high T and high P; Option D: high T and low P.
Now, evaluate each choice using Le Chatelier's principle and basic gas statistics.
Option A — low temperature, high pressure: For an exothermic gas-phase synthesis, lowering temperature favors the forward (exothermic) direction, and increasing pressure favors the side with fewer moles of gas. On the left you have 3 H2 + 1 N2 = 4 moles of gas, and on the right you have 2 NH3 = 2 moles of gas. The forward reaction reduces the total number of gas moles from 4 to 2, so high pressure pushes the equilibrium toward NH3. Simultaneously, the low temperature supports the exothermic formation of NH3. This combination correctly drives the reaction to the right.
Option B — low temperature, low pressure: While the low temperature helps the exothermic forward reaction, lowering pressure would tend to favor the side with more gas moles (the left, with 4 moles), not the right. This combination does not maximize NH3 production and is thus not optimal.
Option C — high temperature, high pressure: High temperature shifts equilibrium toward the endothermic direction (opposite of what we want) and would reduce NH3 yield, since the forward reaction is exothermic. Even with high pressure, the temperature effect would undermine the desired direction, making this choice unattractive for increasing NH3.
Option D — high temperature, low pressure: This configuration strongly disfavors the forward exothermic reaction (both because of high temperature and low pressure). It would push the equilibrium toward reactants, yielding little NH3. Therefore this option is clearly incorrect for producing more ammonia.
In summary, the combination that aligns with Le Chatelier's principle to maximize NH3 production is low temperature and high pressure, which adjust both the temperature (favoring exothermic forward reaction) and the pressure (favoring the fewer-moles product). Consequently, Option A is the correct choice.

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