Endothermic Reaction

[Sydney Rohan 3G]

I am confused about this question. It states:

Consider this system at equilibrium.

A(aq) <-----> B(aq) delta H=−250 kJ/mol

What can be said about Q and K immediately after an increase in temperature?

Q>K because K decreased.

I am confused about this question because I thought that the reaction is endothermic, which I thought meant that it will favor the product, but the answer says that it favors the reactant so I am confused. Can someone please explain this problem, please?

[Amine Adlouni 1L]

The reaction is actually exothermic. When the delta H of a reaction is negative, that means energy was released in the reaction, hence it is exothermic. Hopefully that helps guide your thinking.

[Jonathan Sautter 1J]

Because the (delta)H is negative/ the change in the temperature is negative, this reaction is exothermic. Therefore, heating the reaction will favor the reactants more. However, you are right that if it were to be endothermic, the products would be favored.

[Sunny Hou 2I]

Hi,
So because the delta H value for this reaction is negative, it is actually not an endothermic reaction it is an exothermic reaction. Endothermic reactions are when the enthalpy change is positive which inherently means that there is more energy in the products than the reactants, whereas in exothermic reactions that is the opposite and it means that there is less energy in the product than the reactant.

[Andrew Yim 1K]

Hi,
As others have said, the reaction is exothermic. An easy way to remember it is understanding that change in enthalpy is like change of energy in the system. If it's negative, the system loses energy (releases energy) and is exothermic.

[Harshitha_Pandian_3F]

For this question you need to look at the delta H and for this reaction it is negative. This means that it is an exothermic reaction which means that it favors the reactants.

[oliviahelou]

Because this is an exothermic reaction, the production of reactants will be favored.

[Coraly De Leon]

Hello,
As other mentioned, a negative delta H is a strong indication that the reaction will be exothermic.

[Wilson Zheng 1L]

The negative H value = an exothermic reaction. That means that when energy (heat) is added to the system, the reverse reaction (endothermic) is more likely favored, meaning that there would be more reactant formation.

[Madison Nguyen 3L]

Negative delta means that the heat is being released, and that the reaction is exothermic, meaning that creating products does not require heat. Instead, creating reactants requires heat, meaning that when heat is added, the reactants are favored.

[Hailey Sarmiento 3E]

For me, looking at the delta H value is easies to determine if a reaction is exothermic or endothermic. Exothermic reactions have negative delta H values while endothermic reactions have positive delta H values.

[Srikar_Chintala_1E]

The reaction is actually exothermic because it is releasing energy. Hence, when you increase the temperature, you are favoring the endothermic reaction of the given reaction. Hence, that would be the reverse of the reaction which would lead to more reactants being produced.

[amara ajon 1d]

Hi,
Because this is an exothermic reaction (with a negative enthalpy sign), we know that the reaction favors the reactants.

[405479701]

The delta H of a reaction is negative so energy was released in the reaction. The reaction is exothermic since energy was released.

[Natasha]

Since the delta h is negative the change in temperature is also negative which means the reaction is actually exothermic and not endothermic. This means reactants are favored more over products.

[Diana Avalos]

Since enthalpy(H) is a negative value, this means it's exothermic, meaning the reverse reaction would be favored so reactants are favored.

[Evan L 2B]

This reaction is exothermic because the delta H is negative. When the temperature increases there is going to be a sudden decrease in K because the reaction is now more heavily favoring reactants. However, the current concentration ratios are the same as before the temperature change. Therefore that ratio is Q which is greater than the decreased K.