Chemistry, 21.11.2019 09:31 rubianny03

during a reaction, δh for reactants is −750 kj/mol and δh for products is 920 kj/mol. which statement is correct about the reaction?

it is endothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.
it is endothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed.
it is exothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.
it is exothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed.

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Answer from: sjdswim

Option (b) is the correct answer.

Explanation:

Since energy of reactants is less than the energy of products. Therefore, it means energy is absorbed during the reaction.

As the energy required to break the bonds in the reactants is greater than the energy released when products are formed.

Therefore, it is an endothermic reaction.

Thus, we can conclude that the statement, it is endothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed is correct.

during a reaction, δh for reactants is −750 kj/mol and δh for products is 920 kj/mol. which statemen

Answer from: Isaac0213

The correct answer is :'It is endothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed'.

Explanation:

Endothermic reactions are defined as the reactions in which energy of products is more than the energy of the reactants. In these reactions, energy is absorbed by the system.

The energy required to break the bonds in the reactant is more that the energy released when the products are formed.

The total enthalpy of the reaction $(\Delta H)$ comes out to be positive.

Exothermic reactions are defined as the reactions in which energy of reactants is more than the energy of the products. In these reactions, energy is released by the system.

The energy required to break the bonds in the reactant is less that the energy released when the products are formed.

The total enthalpy of the reaction $(\Delta H)$ comes out to be negative.

ΔH for reactants = -750 kJ/mol

ΔH for products = 920 kJ/mol

ΔH for reactants < ΔH for products

It is endothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed

Answer from: Quest

i'm pretty sure its b i might be wrong though!

Answer from: Quest

Ibelieve the answer is d

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during a reaction, δh for reactants is −750 kj/mol and δh for products is 920 kj/mol. which statemen...