1 multiple answer 10 points given the reaction below, when co₂ (g) is removed, this will occur. check all…

1 multiple answer 10 points given the reaction below, when co₂ (g) is removed, this will occur. check all that apply. ch₄ (g) + 2o₂ (g) ⇌ co₂ (g) + 2h₂o (l) + heat reaction will shift toward products less o₂ (g) is consumed in the reaction more h₂o (l) is produced reaction will shift toward reactants. more co₂ (g) is produced

1 multiple answer 10 points given the reaction below, when co₂ (g) is removed, this will occur. check all that apply. ch₄ (g) + 2o₂ (g) ⇌ co₂ (g) + 2h₂o (l) + heat reaction will shift toward products less o₂ (g) is consumed in the reaction more h₂o (l) is produced reaction will shift toward reactants. more co₂ (g) is produced

Answer

Explanation:

Step1: Apply Le - Chatelier's principle

According to Le - Chatelier's principle, when a system at equilibrium is disturbed, the system will shift to counteract the change. In this exothermic reaction $CH_4(g)+2O_2(g)\rightleftharpoons CO_2(g) + 2H_2O(l)+\text{Heat}$, removing $CO_2(g)$ is a disturbance.

Step2: Determine the direction of the shift

Since $CO_2$ is a product, removing it will cause the reaction to shift to produce more $CO_2$. So the reaction will shift towards the products. When the reaction shifts towards the products, more reactants ($CH_4$ and $O_2$) will be consumed and more products ($CO_2$ and $H_2O$) will be produced.

Answer:

  • Reaction will shift toward products
  • Less $O_2(g)$ is consumed in the reaction (False)
  • More $H_2O(l)$ is produced
  • Reaction will shift toward reactants. (False)
  • More $CO_2(g)$ is produced