Methanol is manufactured by the following exothermic reaction. CO (g) + 2H2 (g) ⇌ CH3OH (g) Which pair of changes will favour the forward reaction?[Fill in the blank]

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BlackTom AI · Accepted Answer

First, restate the problem to ensure understanding: the reaction CO(g) + 2 H2(g) ⇌ CH3OH(g) is exothermic, and we are asked which changes will favour the forward reaction.

Option a: Increased pressure and temperature
- Increasing pressure generally favours the side with fewer gas moles. Since the forward reaction converts 3 moles of gas (1 CO + 2 H2) into 1 mole of CH3OH, higher pressure would tend to push toward the product, which is good. However, increasing temperature for an exothermic reaction typically favours the reverse reaction because heat acts as a product in the forward direction. The combined effect here is mixed: pressure would push forward, but higher temperature would push backward, making this choice not consistently favorable for the forward direction.

Option b: Decreased pressure and temperature
- Decreasing pressure shifts equilibrium toward more gas moles, i.e., toward reactants, which disfavors the forward reaction. Additionally, lowering the temperature would favor the forward reaction for an exothermic process, but the detrimental effect of reduced pressure dominates here, so overall this choice does not correctly favour the forward direction.

Option c: Decreased pressure and increased temperature
- Decreasing pressure again pushes toward more gas molecules (reactants), disfavoring the forward reaction. Increasing temperature, while it would favor the reverse for an exothermic reaction, does not compensate for the pressure effect. Therefore this option does not favor the forward direction.

Option d: Increased pressure and decreased temperature
- This combination aligns with both key factors: increasing pressure favours the side with fewer gas moles, i.e., the product CH3OH. Decreasing temperature also favours an exothermic forward reaction because the system is driven to release heat as it forms more product. Together, these changes strongly promote the forward reaction.

In summary, the most favorable conditions for pushing the equilibrium toward CH3OH production are those that increase pressure (to exploit the lower gas-mole count on the product side) and decrease temperature (to maximize exothermic gain). This makes the fourth option the correct pairing for promoting the forward reaction.

Methanol is manufactured by the following exothermic reaction. CO (g) + 2H2 (g) ⇌ CH3OH (g) Which pair of changes will favour the forward reaction?[Fill in the blank]

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Methanol is manufactured by the following exothermic reaction. CO (g) + 2H2 (g) ⇌ CH3OH (g) Which pair of changes will favour the forward reaction?[Fill in the blank]

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类似问题

Chemical equilibrium is the state where chemical reactions are in balance and no longer occurring.

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Which of the following statements concerning equilibrium constants is true?

Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are

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Consider the equilibrium system C(s) + CO2(g) ⇔2CO(g) If C is removed, the equilibrium will _, and if CO is added, the equilibrium will _.