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Direction

Posted: Thu Jan 09, 2020 3:20 pm
by Jarrett Peyrefitte 2K
How does the value of the reaction quotient allow the direction of non-equilibrium reaction to be predicted?

Re: Direction

Posted: Thu Jan 09, 2020 3:22 pm
by Connie Chen 1E
If Q<K, then we know that the reaction will favor the forward reaction because there is not enough product for the reaction to be at equilibrium.
If Q>K, then we know the reaction will favor the reverse reaction because there is not enough reactant for the reaction to be at equilibrium.

Re: Direction

Posted: Thu Jan 09, 2020 3:22 pm
by Kate Osborne 1H
if Q is less than K then the reaction will proceed in the forward direction, while if Q is greater than K the reaction will proceed in the reverse direction.

Re: Direction

Posted: Thu Jan 09, 2020 3:24 pm
by nicole-2B
Connie Chen 1E wrote:If Q<K, then we know that the reaction will favor the forward reaction because there is not enough product for the reaction to be at equilibrium.
If Q>K, then we know the reaction will favor the reverse reaction because there is not enough reactant for the reaction to be at equilibrium.

Thanks for clarifying!!

Re: Direction

Posted: Sun Jan 12, 2020 5:18 pm
by Emily Lo 1J
If the Q value is less than K, then there is more reactant than there is product in the reaction, and the direction which the reaction favors it forward.
If the Q value is greater than K, then there is more product than there is reactant in the reaction, and the direction which the reaction favors is reverse.