Quotient

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Matthew Lee 3L
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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
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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
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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
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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

Victor Qiu 1C
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Re: Quotient

Postby Victor Qiu 1C » Sun Jan 17, 2021 8:23 am

Basically, K is the relative ratio of products to reactants when the reaction is at equilibrium, while Q is the relative ratio of products to reactants at a given instant (the reaction might not be at equilibrium).

Jessica Katz
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Re: Quotient

Postby Jessica Katz » Sun Jan 17, 2021 8:26 am

Q is the relative concentrations at a given time, and k is only used when at equilibrium. so they are used in comparison to determine if more products or more reactants are going to be made in order for the Q to equal K.

Daniela Santana 2L
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Re: Quotient

Postby Daniela Santana 2L » Sun Jan 17, 2021 7:56 pm

Q is the reaction quotient, K is the equilibrium constant. Q can be calculated at any time whereas K can only be calculated at equilibrium. Hope this helps!

Simran Bains 2C
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Re: Quotient

Postby Simran Bains 2C » Sun Jan 17, 2021 8:07 pm

Q is the reaction quotient, whereas K is the reaction quotient at equilibrium specifically.

Griffin G
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Re: Quotient

Postby Griffin G » Sun Jan 17, 2021 8:21 pm

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

Hannah Lechtzin 1K
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Re: Quotient

Postby Hannah Lechtzin 1K » Sun Jan 17, 2021 8:24 pm

Q and K are almost the same. The only difference is the K is when the reaction is at equilibrium while Q is not.

rhettfarmer-3H
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Joined: Wed Sep 30, 2020 9:59 pm

Re: Quotient

Postby rhettfarmer-3H » Sun Jan 17, 2021 11:34 pm

Q is basically K at a time of the reaction that is not an equilibrium. Use the term Q to basically indicate that it is not at equilibrium. Therefore, they are entirely the same, it helps to describe the state of the reaction.

SashaAnand2J
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Joined: Wed Sep 30, 2020 9:37 pm

Re: Quotient

Postby SashaAnand2J » Mon Jan 18, 2021 2:06 am

Hi Matthew!

Q is similar to K, in that the equation setup for both are identical, however, the concentrations that are substituted into the equations are different. Q is when the concentrations of the reactant and product are not at equilibrium. K always uses equilibrium constants.

Carly_Lipschitz_3H
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Joined: Wed Sep 30, 2020 9:56 pm

Re: Quotient

Postby Carly_Lipschitz_3H » Thu Jan 21, 2021 5:09 pm

K is the equilibrium constant, and Q is the reaction quotient. They are both calculated the same way, but K stays constant. Q does not stay constant since it can be taken at any time. Q doesn't specifically need to be taken when the reaction is at equilibrium like K is. When Q<K, the forward reaction is favored, and when Q>K, the reverse reaction is favored.


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