Module 1A #12

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Chloe Shamtob 2H
Posts: 105
Joined: Wed Sep 30, 2020 9:55 pm

Module 1A #12

Postby Chloe Shamtob 2H » Mon Jan 04, 2021 2:17 pm

12. For a chemical reaction that has reached equilibrium which statement is false?

A. The forward reaction rate is the same as the reverse reaction rate.

B. No matter what combination of concentrations of reactants and products we start with, the reaction will reach equilibrium.

C. There is no reaction occurring.

D. The concentrations of the reactants and products do not change.

E. None of the above

What's the answer to this question? Is it C because a reaction is still occurring? Or do reactions not occur at equilibrium?

Ria Nawathe 1C
Posts: 98
Joined: Wed Sep 30, 2020 9:39 pm
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Re: Module 1A #12

Postby Ria Nawathe 1C » Mon Jan 04, 2021 2:19 pm

You're correct, C is false! At equilibrium, the forward and reverse reactions do still occur, just at the same rate.

Breanna Ouyang 1I
Posts: 92
Joined: Wed Sep 30, 2020 9:48 pm

Re: Module 1A #12

Postby Breanna Ouyang 1I » Mon Jan 04, 2021 6:22 pm

The answer is C because it's at dynamic equilibrium (not static equilibrium), so the reactions are just occurring at equal rates.


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