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In this video, we're going to be talking about endothermic reactions.
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So an endothermic reaction, if you don't remember, is a reaction that requires heat from the surroundings.
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So a system will essentially absorb heat from its surroundings.
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So a physical example could be in an ice cube melting, right? so it's absorbing heat from its surroundings.
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I have here a chemical, generic chemical equation for how this type of reaction occurs.
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So we have two reactants, a and b, and we need to input heat, right, with the reactants to form this product c or any other products.
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And it turns out for endothermic reactions that the change in enthalpy, so remember, enthalpy is an energy like property, it's a state function.
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And this change in enthalpy for this reaction is always going to be positive.
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And the reason being is that the bonds broken, right, we need to input.
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Put more energy to break the bonds than the amount of energy that we yield.
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And so the bonds broken is going to have a higher magnitude than the energy that we form.
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Remember, bonds broken is always positive because we input energy.
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When we form bonds, we're going to release heat.
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We're going to create energy.
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So here's an energy diagram for an endothermic reaction.
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We have potential energy on the y.
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Axis and then we have the reaction progressing in the x -axis...