Unequal Reactant

[VahagnAldzhyan]

What happens when you have more reactants than products? Does the equilibria sign lean to the left.

[Sarah Rutzick 1L]

When there are more reactants than products, the equilibrium sits to the left. This is because the denominator of the K expression is larger than the numerator, which leads to a K value that is less than one meaning that the equilibrium sits to the left.

[John Huang 1G]

I believe the equilibria sign would lie to the right actually. When you have more reactants than products, the calculated Reaction Quotient (Q) value will be less than one, not the K value. So because the Q value would be less than the K value, the equilibrium would lie to the right because the forward reaction is favored in this case.

[AtreyiMitra2L]

When there are more reactants than products, the equilibrium sits to the left. This is because the denominator of the K expression is larger than the numerator, which leads to a K value that is less than one meaning that the equilibrium sits to the left.

Actually, K is actually not affected by the amount of reactants and products as seen by 11.1 C. As seen by 11.1 B, increasing the reactants would shift the reaction to the right.