Chemistry, 08.11.2019 04:31 karamalqussiri478

The activation energy of an endothermic reaction
1. must be greater than the required δh
2.must be less than the required δh
3.must be equal to the required δh
4.is not needed for the required δh

Answers: 2

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Endothermic reactions are reactions that require heat in the course of the process. The heat of reaction in this case is positive which means the energy of the products is greater than the energy of the reactants. In this case, the answer to this problem would have to be 1. must be greater than the required ΔH

Answer from: laurentsupreme

3. The difference between the potential energy of the products and the potential energy of reactants.

Answer from: gokusupersaiyan12345

The correct answer is Option 3.

Explanation:

The net energy absorbed or released in a chemical reaction is known as the total enthalpy change of the reaction. It is written as $\Delta H_{rxn}$

The formula used to calculate total enthalpy of the reaction is:

$\Delta H_{rxn}=\sum H_{products}-\sum H_{reactants}$

where,

$H_{products}$ = Potential energy of the products

$H_{reactants}$ = Potential energy of the reactants

Hence, the correct answer is Option 3.

Answer from: 231agoad

The correct answer is Option 3.

Explanation:

The net energy absorbed or released in a reaction is known as total enthalpy change of the reaction. It is designated as $\Delta H_{rxn}$

It is defined as the difference between the total potential energy of the products and the total potential energy of the reactants. The equation for this is given by:

$\Delta H_{rxn}=\sum \Delta H_{products}-\sum \Delta H_{reactants}$

where,

$\Delta H_{products}$ = Total potential energy of the products

$\Delta H_{reactants}$ = Total potential energy of the reactants

Hence, the correct answer is Option 3.

Answer from: genyjoannerubiera

A reaction profile includes the activation energy , which is the minimum energy needed by particles when they collide for a reaction to occur. The activation energy is shown as a 'hump' in the line, which: starts at the energy of the reactants.

I hope this helps! :)

Answer from: tiffcarina69

must be greater than the required ΔH

Explanation:

The activation energy is the minimum extra amount of energy required by reactant molecules to undergo a reaction.

For both exothermic and endothermic reactions we need activation energy.

Enthalpy is the energy difference between products and reactants.

For endothermic reactions, enthalpy is positive as the energy of products is more than the energy of reactants.

As activation energy will be greater than the energy of both the reactants and products, so it must be greater than the enthalpy of reaction.

Answer from: bacchus6663

The activation energy of an endothermic reaction must be greater that the required ΔH

Explanation:

In chemistral reaction, when you have endothermic reaction, the energy of reactives must be less that energy of products, because we need energy to make them. As we need it, that's why we say that it is endothermic reaction, remember that if you want to calculate ΔH, you should do a substraction between, activation energies.

Answer from: sammy16940

C. The differencece between the potential energy of the products and the potential energy of the reactants

Answer from: AADJ4

I think the correct answer would be the third option. The activation energy of an endothermic reaction should be equal to the required ΔH. The activation energy is the energy needed to be achieved or reached in order for a reaction to occur. So, enthalpy change should be equal or greater than that of the activation energy.

Answer from: taijaababy

This is true, an endothermic reaction will have an AE greater than the deltaH value

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The activation energy of an endothermic reaction
1. must be greater than the required δh

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