Is this false? I think so because when Q > K the rxn moves towards the reactants

Question

Is this false? I think so because when Q > K the rxn moves towards the reactants so less products would be formed right?

Also,

A chemical reaction will reach equilibrium when the limiting reactant is used up.

This should also be false because equilibrium wouldn't be reached if one of the reactants was used up, correct?

Thanks.

If Q > K, more products need to be formed as the reaction proceeds to equilibrium. Is this false? I think so because when Q > K the rxn moves towards the reactants so less products would be formed right? Also, A chemical reaction will reach equilibrium when the limiting reactant is used up. This should also be false because equilibrium wouldn't be reached if one of the reactants was used up, correct? Thanks.

Explanation / Answer

a)

If Q> K then products form reactants to equilibrate. TRUE

Q = [Actual Concentration of Products] / [Actual concentration of Reactants]

K = [Concentration of Products in Equilibrium] / [Concentration of Reactants in Equilibrium]

When Q>K, there are more products than reactants.

To decrease the amount of products, the reaction will shift to the left and produce more reactants.

B)

"A chemical reaction will reach equilibrium when the limiting reactant is used up." FALSE

The equilibrium does not depend on the limiting reactant. Actually, the reaction will simply stop, searching for further "equiilbrium" conditions, but since concentrations can not be changed, there will be no other effects of cocnetration with time. One will think this reaction is in equilbirum but in reality it is because there is no more reactant to continuewith the final concentration of equilibrium

So, you are correct in both of them!

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