Value of Q

[Joshua Eidam 2A]

When looking at the equation w(max)= , I was confused as to what Q is? I understand it is the reaction quotient but how exactly do you calculate that?

[Katie Nye 2F]

You calculate Q in a similar way to the equilibrium constant! It is the concentration of the products raised to their coefficient divided by the reactants raised to their coefficients. the only difference is for Q, the reaction is not at equilibrium.

[Charlie Russell 2L]

As Katie said! Also, if Q<K, reaction will continue to shift towards products, if Q>K, reaction will shift towards reactants.

[Stephen Min 1I]

Q would represent which direction the equation shifts and it is not at equilibrium, as opposed to K.

[Wasila Sun 2I]

Q is calculated the same way as the equilibrium constant K. So we can figure this out by taking the Q=[products]/[reactants]. If Q=K then the system is at equilibrium.

[Grecia Velasco 1G]

Q is the quotient reactant that we learned for and before Midterm 1! It is [P]/[R] like K but NOT at equilibrium.
To compare Q and K use le chatelier's princple:
Q<K; will shift to products so -DeltaG and spontaneous
Q=K; equilibrium
Q>K; will shift to reactants so +DeltaG and spontaneous in the reverse rxn

[Gian Boco 2G]

Q is the ratio of concentrations of the products over the reactants with respect to their stoichiometric coefficients.

[Kathy_Li_1H]

Hi! The value of Q is the reaction quotient, which can be solved the same as you calculate K (the equilibrium constant).

[Vince Li 2A]

Q is the same thing as K, only that the reaction has not reached equilibrium. The problem should give the values of the concentrations for the products and reactants, so you can calculate Q knowing the balanced equation. Depending on the value of Q, the value of the Gibbs free energy will determine if more products or more reactants need to be formed to reach K.

[Mackenzie Van Val 3E]

You calculate Q in the same way you calculate K; it is the concentration of the products, to the power of their stoichiometric coefficient, over the concentration of the reactants to their stoichiometric coefficients.

[LReedy_3C]

Concentration of products (to the power of their coefficients) over concentrations of reactants (to the power of their coefficients), or I think you can do the same with partial pressures. It's the same as calculating the equilibrium constant the system's just not at equilibrium

[Andersen Chu 2H]

Q is simply the reaction quotient from the chemical equillibrium unit. It is the ratio of concentrations of products to reactants which is calculated from (concentration of product)^n x (concentration of product 2)^n etc. divided by (concentration of reactant)^n x (concentration of reactant 2)^n. Where n is the number of moles of the corresponding species

[Kiara Phillips 3L]

Q is what we call K or the equilibrium but Q is K but not at equilibrium and its used to identify which way the reaction will proceed.

[Sean Wang 1F]

Q is calculated the same way as K, just Q is the constant when not at equilibrium.

[Isabella Cortes 2H]

Q is calculated the same way that we find K. It is the concentration of products over the concentration of reactants both raised to the power of their stoichiometric coefficients when a reaction is not at equilibrium.

[Keshav Patel 14B 2B]

Q is the equilibrium constant. If you have molar concentrations of the reactants and products you can make it reactants/products and put them to the power of number of moles. That gives you the Q value.

[Colin Squire 3B]

Finding the value of Q is the same as finding the equilibrium constant K. We divide the partial pressure or the molar concentrations with the products on top and the reactants on the bottom with the coefficients as exponents.

[Jaden Kwon 3C]

Calculating Q, the reaction quotient, is the same process as calculating K, the equilibrium constant, which we learned earlier. You can do this by taking the concentrations/partial pressures of the products and raising each one to their stoichiometric coefficients and dividing that by the concentrations/partial pressures of the reactants raised to each of their stoichiometric coefficients. You are usually given the values of the concentrations/partial pressures.

[Ansh Patel 2I]

Q is the same concept as K but Q is not at equilibrium and it's used to determine which way the reaction will proceed.

[Ellison Gonzales 1H]

How do you know to use the equation with Q instead of K based off the question? If the question is asking you to compare something to a K value, is that when we use this equation with the Q?

[DPatel_2L]

It is calculated in the same way, but it is just not at equilibrium.