Direction
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Direction
How does the value of the reaction quotient allow the direction of non-equilibrium reaction to be predicted?
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Re: Direction
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.
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.
Last edited by Connie Chen 1E on Thu Jan 09, 2020 3:22 pm, edited 1 time in total.
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Re: Direction
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
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!!
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Re: Direction
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.
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.
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