Help me understand this Q

[prsndwg]

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help me out here please. I picked C and it was Wrong 😕

 

[Bizzlers]

help me out here please. I picked C and it was Wrong 😕

Answer: A

Increasing the temperature for the reaction will increase both forward and reverse reactions as demonstrated by the arrhenius equation. Increasing the temperature will increase the forward and reverse reaction rate constants, k and k' respectively.

Do not confuse this with the reaction's equilibrium.

 

[prsndwg]

thanks for your responses.. but how would I distinguish between the equilibrium and the kinetics as you explained. any hints?

 

[Bizzlers]

Anything that asks for rates or rate constants is usually kinetics.

If it asks for which side the equation would it be more favorable for...then its usually a chemical equilibrium question.

 

[UCB05]

Basically just keep in mind that rate will pretty much always go up with an increase in temperature.

Higher temperature = more energy/faster collisions = more reactions = higher rate of reaction

Of course rate only deals with a single direction reaction. Equilibrium describes the relationship between two opposite reactions. An increase in temperature implies both the forward AND reverse reactions increase in rate. However, the endothermic reaction direction will benefit MORE from the temp increase than the reverse, exothermic reaction. This is why the equilibrium shifts. Though both forward and reverse reactions speed up, one side benefits more from the temperature change, so the new equilibrium ratio is different.

The question specifically asks about rate, so you should immediately conclude that both forward and reverse reactions increase rate. The equilibrium shifts toward the reactants.