Activation energy question

[datattack]

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Could someone please help explain this question:

Decreasing the activation energy of the forward reaction will do what to the reverse reaction rate?

A. Decrease the rate
B. Increase the rate
C. Have no effect
D. Effect the equilibrium
E. Make the reaction reach equilibrium slower

The answer is B. Increase the rate


[[[Does decreasing the activation of the forward reaction likewise decrease the activation energy of the reverse reaction? Which would provide a lower activation for it and increase its rate?]]]

Thank you!

 

[Maygyver]

Hey, hopefully this helps: think of it by drawing a diagram. So, think of the typical drawing with the starting material on one side and the product on the other with a uphill intermediate. The energy of activation (EA) will be the distance from A to the intermediate. If you lower this, it will also lower the distance between B and the intermediate, so that reaction will therefore happen more often as well. Make sense?

 

[DoCt0rPeTe]

The energy of activation ultimately determines how fast the rxn will go.

You walk from your house, point A to the store, point B. But on the way, you tie your shoes slowly (activation energy).

Say now that a catalyst makes you tie them faster. You'll get to the store faster (A---> B)
and you'll also get back faster (B---->A)


It's not a perfect example but it may help you conceptualize it.

 

[datattack]

Yep, it makes a lot more sense. Thank you!