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Hanniel U 2B
Posts: 76
Joined: Fri Sep 28, 2018 12:16 am


Postby Hanniel U 2B » Tue Jan 08, 2019 10:10 pm

Can someone please help me with 5G.11 7th edition?

Venya Vaddi 1L
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Joined: Fri Sep 28, 2018 12:16 am
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Re: Q

Postby Venya Vaddi 1L » Wed Jan 09, 2019 2:19 pm

Q is written the same way as K is. Q=[products]/[reactants] and both solids and liquids are excluded from the expression.

Katie Frei 1L
Posts: 64
Joined: Fri Sep 28, 2018 12:27 am

Re: Q

Postby Katie Frei 1L » Wed Jan 09, 2019 2:36 pm

To find Q, or the reaction quotient, you would need to use the same equation used to find K, or the equilibrium constant. Also only include gases and aqueous phases in your equation to find Q.

Anusha 1H
Posts: 65
Joined: Fri Sep 28, 2018 12:15 am

Re: Q

Postby Anusha 1H » Wed Jan 09, 2019 2:45 pm

Use the same approach you use to find K (products/reactants).

a) for example would be -- Q = 1/(P BCl3)^2

Hai-Lin Yeh 1J
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Re: Q

Postby Hai-Lin Yeh 1J » Wed Jan 09, 2019 4:55 pm

How did you get 1 in the numerator? I know that the molar concentration of a pure substance (solid or liquid) does not change in a reaction so they are not included, but where did you get the 1 from?

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

Re: Q

Postby Karyn Nguyen 1K » Wed Jan 09, 2019 4:58 pm

Can someone explain what exactly Q is? I know that it is the reactant quotient but I don't get why Q and K wouldn't always equal each other if they have the same formula [P]/[R]?

Posts: 76
Joined: Fri Sep 28, 2018 12:24 am

Re: Q

Postby EllerySchlingmann1E » Wed Jan 09, 2019 5:03 pm

Q and K are not always the same because Q represents [P]/[R] at any time in the reaction while K represents that ratio only when the reaction is at equilibrium. If Q does not equal K, we know that the equation is not at equilibrium.

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