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The reaction represented above goes essentially to completion. The reaction takes place in a rigid, insulated vessel that is initially at 600 K Which of the following statements about the bonds in the reactants and products is most accurate?

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Answer:

Option C.

Explanation:

The reaction is a gaseous reaction. Lets look at the reaction once again:

CH₃OH (g) → CO(g) + 2 H₂ (g)  ΔH = +91 kJ/mol

As we can see from the reaction above, the process is an endothermic process (positive sign). It means that the reaction must absorb as much heat as possible.

According to Le Chatelier's principle, the creation will favor product formation.For a gaseous system, the reaction will tend to reduce the heat of the system by absorbing more heat.  Hence option C

When the closed arrangement consumes energy from the enclosing environment then the process is an endothermic reaction.

The gaseous reaction in the question is:

CH₃OH (g) → CO(g) + 2 H₂ (g)    , ΔH = + 91 kJ/mol

The correct answer is:

The total of the bond enthalpies of the reactant bonds are smaller than the quantity of the bond enthalpies of the bonds of the product.

This can be explained as:

  • Since the result has a positive sign the reaction is endothermic.

  • The total of the bond enthalpies of the reactant bonds will be less than the total of the bond enthalpies of the product linked.

  • This system will absorb heat from the surroundings.

  • According to a principle, this equation will support product formation.

Therefore, the reactants will consume energy from the surroundings and will form results.

To learn more about Endothermic reaction refer to the link:

https://brainly.com/question/15872460