K and Q

[Brandon Tao 1K]

What is the difference between K and Q if they are calculated the same way?

[sbeall_1C]

K and Q are calculated in the same way, except that K uses the values from equilibrium and Q uses initial conditions/conditions not at equilibrium. You can use the value of Q to determine which way the the reaction will proceed to reach equilibrium!

[Sanjana Borle 2K]

If you compare Q to K, you can determine whether the reaction is going go to in the forward or reverse reaction to reach equilibrium.

[Sidharth D 1E]

If Q < K, at some time during the reaction, then the forward reaction is favored.
If Q > K, at some time during the reaction, then the reverse reaction is favored.

[Dan M -3E]

K is the equilibrium constant. Q is the same calculation as K, but when the reaction isn't at equilibrium. From the value of Q, you can tell if the reaction is making more products or reactants.

[CalvinTNguyen2D]

K is calculated when the reaction is at equilibrium, but Q is not. Q is a great indicator to figure out which way the reaction is favored.

[saigorijavolu2k]

Q is calculated when the reaction is not at equilibrium and K is. K remains the same.

[zfinn]

Q is the calculation of a system not at equilibrium while K is the calculation of a system at equilibrium (the equilibrium constant).

[Hope Hyland 2D]

Q is the reaction quotient, whereas K is the equilibrium constant. While they are both ratios of product to reactant, K represents the ratio when the reaction is at equilibrium, or when the forward rate of the reaction is equal to the reverse rate (products are being formed at the same rate as reactants). On the other hand, Q is simply the ratio of product to reactant at any given time during the reaction.

[Viviana Velasquez]

K is the equilibrium constant and Q tells you the constant of the equation when it is not at equilibrium. Q helps you judge whether it is a forward or backwards reaction.

[505306205]

K and Q are different because K represents the reaction at equilibrium whereas Q represents the reaction at a point other than at equilibrium.