What happens if Q is greater than K?
Q < k:="" when="" q="">< k,="" there="" are="" more="" reactants="" than="" products="" resulting="" in="" the="" reaction="" shifting="" right="" as="" more="" reactants="" become="" products.="" q=""> K: When Q > K, there are more products than reactants resulting in the reaction shifting left as more products become reactants.
Why is it useful to compare Q with K?
By comparing Q and K, we can predict whether a reaction will shift towards the reactants or the products to reach equilibrium. This understanding is fundamental in many areas of chemistry, including industrial processes, where controlling the direction of chemical reactions is often crucial.
How does Q relate to G?
ΔG is related to Q by the equation ΔG=RTlnQK. If ΔG < 0,="" then="" k=""> Q, and the reaction must proceed to the right to reach equilibrium. If ΔG > 0, then K < q,="" and="" the="" reaction="" must="" proceed="" to="" the="" left="" to="" reach="">
What is the relationship between K and equilibrium?
The larger the K, the farther the reaction proceeds to the right before equilibrium is reached, and the greater the ratio of products to reactants at equilibrium. If K is less than 0.001, it is considered small and it will be mostly reactants.
How is Q different from K?
When Q is less than K is it spontaneous?
What to do if Q is less than K?
What does it mean when Q is less than K in chemistry?
What is the difference between K value and Q value in chemistry?
What is Q in equilibrium?