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Consider the following exothermic process at equilibrium:

CO(g)+H2O(g)⇌CO2(g)+H2(g)

Which of the following changes would increase the amount of H2(g) present in the equilibrium mixture?

Consider the following exothermic process at equilibrium:


Which of the following changes would increase the amount of present in the equilibrium mixture?

decrease the temperature
increase [CO2]
increase [CO]
increase the volume of the container in which the reaction occurs.
more than one of the above
(Answer is not increase [CO])

Respuesta :

dsdrajlin

For the given exothermic process at equilibrium, an increase in the concentration of CO would increase the amount of H₂.

How is equilibrium affected by changes?

When a perturbation is done on a system at equilibrium, it shifts its equilibrium position to counteract the perturbation.

Let's consider the following exothermic process at equilibrium.

CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)

Which of the following changes would increase the amount of H₂(g) present in the equilibrium mixture?

  • decrease the temperature. NO. For an exothermic reaction, a decrease in the temperature will shift the equilibrium towards the reactants.
  • increase [CO₂]. NO. This would shift the equilibrium towards the reactants.
  • increase [CO]. YES. This would shift the equilibrium towards the products.
  • increase the volume of the container in which the reaction occurs. NO. This wouldn't affect the equilibrium since the number of gaseous moles is the same on both sides.
  • more than one of the above. NO.

For the given exothermic process at equilibrium, an increase in the concentration of CO would increase the amount of H₂.

Learn more about equilibrium here: https://brainly.com/question/2943338

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