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Postby 504909207 » Fri Jan 11, 2019 9:49 pm

Why does heat prefer endothermic reactions?

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Re: Endothermic

Postby madisondesilva1c » Fri Jan 11, 2019 10:33 pm

During lecture, Dr. Lavelle noted that endothermic reactions require heat. Therefore, in order to proceed they will need heat due to requiring energy due to products from reactants having a positive enthalpy value. Looking at graphs of endothermic vs. exothermic could help you understand a visual.

Matthew Tran 1H
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Re: Endothermic

Postby Matthew Tran 1H » Sat Jan 12, 2019 12:39 am

Another way to think about it is that for endothermic reactions, heat is a "reactant", and for exothermic reactions, heat is a "product." You can then apply the same concepts that we used to determine the change when reactants and products were added.

Tony Ong 3K
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Re: Endothermic

Postby Tony Ong 3K » Sat Jan 12, 2019 1:11 am

you can also think of it in the sense that endothermic reactions REQUIRE energy and thus can be in the form of heat where exothermic reaction RELEASES energy, which can be in the form of heat as well.

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Re: Endothermic

Postby katie_sutton1B » Sat Jan 12, 2019 8:54 am

Endothermic reactions requires heat, and can basically be included as a reactant of the formation. Exothermic releases heat, and can be thought of as a product.

Cade Okohira 4K
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Re: Endothermic

Postby Cade Okohira 4K » Sat Jan 19, 2019 1:53 am

In chemical reactions, chemical bonds are either broken or formed. Generally, when chemical bonds are formed, heat is released, and when chemical bonds are broken, heat is absorbed. So, heat prefers endothermic reactions because the system gains heat. Meanwhile, a chemical reaction is exothermic if heat is released by the system into the surroundings.

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Re: Endothermic

Postby KHuang1L » Sat Jan 19, 2019 12:34 pm

Heat is required in endothermic reactions, so adding heat will further the reaction.

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