Q  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Jesse_torres2H
Posts: 41
Joined: Thu Jul 27, 2017 3:00 am

Q

Postby Jesse_torres2H » Mon Nov 27, 2017 12:23 pm

Today in lecture Dr. Lavelle was talking about finding Q, what does Q actually represent I was a little confused.

Cali Rauk1D
Posts: 51
Joined: Fri Sep 29, 2017 7:03 am

Re: Q

Postby Cali Rauk1D » Mon Nov 27, 2017 12:31 pm

q is the quantity of heat

Christine Wastila 1H
Posts: 61
Joined: Fri Sep 29, 2017 7:04 am

Re: Q

Postby Christine Wastila 1H » Mon Nov 27, 2017 4:02 pm

Q is the reaction quotient. By comparing this value to K, we can determine how the reaction will progress. If Q<K, the formation of products will be favored. If Q>K, the formation of reactants will be favored. If Q=K, then the reaction is at equilibrium.

Michelle Pham_3H
Posts: 26
Joined: Fri Sep 29, 2017 7:07 am

Re: Q

Postby Michelle Pham_3H » Tue Nov 28, 2017 1:07 am

To add on to what was said earlier, Q is the ratio of the products to reactants in a given instant, while K is this ratio at equilibrium.

Nehal Banik
Posts: 64
Joined: Thu Jul 13, 2017 3:00 am

Re: Q

Postby Nehal Banik » Tue Nov 28, 2017 1:25 pm

Q is the ratio of the products and the reactants with the initial concentrations or whatever data the problem gives you, whereas K is the equilibrium concentration for the reaction, which does not change with changes to pressure and concentration, however it does change with change to temperature.

Shreya Ramineni 2L
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

Re: Q

Postby Shreya Ramineni 2L » Mon Dec 04, 2017 3:27 pm

Q is the reaction quotient and represents the ratio of products and reactants at any point within reaction. When compared to K it provides insight into how the reaction will go.

Madeline Musselman 3H
Posts: 25
Joined: Fri Sep 29, 2017 7:07 am

Re: Q  [ENDORSED]

Postby Madeline Musselman 3H » Sun Dec 10, 2017 10:52 am

Q can be used to compare to K in terms of seeing if a reaction is at equilibrium or not.

Danny Elias Dis 1E
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Re: Q

Postby Danny Elias Dis 1E » Thu Jan 10, 2019 10:31 am

To expand and clarify, Q and K are calculated the same way. The only difference is the value found for K will be the constant value at equilibrium. Using the same math, you can calculate the reaction quotient (Q) but for any point in the reaction (not necessarily when the reaction is at equilibrium).


Return to “Non-Equilibrium Conditions & The Reaction Quotient”

Who is online

Users browsing this forum: No registered users and 3 guests