Quotient

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Matthew Lee 3L
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

Quotient

Postby Matthew Lee 3L » Thu Nov 30, 2017 12:05 am

Is Q basically the same thing as K or are they different?

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

Re: Quotient

Postby Nehal Banik » Thu Nov 30, 2017 12:10 am

Q itself, is the reaction quotient for the reaction given with whatever initial numbers that you are given. Whereas K is the equilibrium quotient, which is the ratio of the concentration/partial pressure of the products and reactants.

Lily Guo 1D
Posts: 64
Joined: Fri Sep 29, 2017 7:03 am

Re: Quotient

Postby Lily Guo 1D » Thu Nov 30, 2017 12:22 am

Q is the reaction quotient, while K is the equilibrium quotient. They both follow the same expression -- the product of the concentrations or partial pressures of each product raised to the power of its stoichiometric coefficient over the product of the concentrations or partial pressures of each reactant raised to the power of its stoichiometric coefficient. However, when calculating Q, you can use the concentrations or partial pressures of the reactants and products at any point in the reaction. When calculating K, you use the equilibrium concentrations or partial pressures, not just any concentrations or partial pressures.

aaron tang 2K
Posts: 49
Joined: Thu Jul 27, 2017 3:01 am

Re: Quotient

Postby aaron tang 2K » Thu Nov 30, 2017 11:57 pm

Q is the quotient which is the for when the reaction is given with whatever initial values are given. K is the equilibrium quotient which is the ratio of the concentration and partial pressure of the reactants and products


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