What is the effect of increasing the temperature of an endothermic reaction mixture at equilibrium? Of decreasing the temperature?
We use heat,
In an exothermic reaction, heat is evolved:
And in an endothermic reaction, heat is absorbed:
Of course, at a different temperature a new equilibrium might pertain, but the initial change, the initial response of the equilibrium (which is after all only what Le Chatelier's principle predicts!) is to resist the temperature change (i.e. the external perturbation), by shifting the direction of the equilibrium appropriately to absorb or evolve heat.
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Increasing the temperature of an endothermic reaction mixture at equilibrium shifts the equilibrium position in the direction of the endothermic reaction, favoring the formation of products. Decreasing the temperature shifts the equilibrium position in the direction of the exothermic reaction, favoring the formation of reactants.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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- For the reaction #"B"_2"H"_6(g) + 6"Cl"_2(g) -> "B"_2"Cl"_6(g) + 6"H"_2(g)#, if #"0.252 mols Cl"_2# reacts with #"0.111 mols B"_2"H"_6#, and #DeltaH_(rxn)^@ = -"1396 kJ"#, what is the heat of reaction?
- What are the values of #DeltaH# and #DeltaS# for the change from gaseous to liquid #H_2O#?

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