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Q VS. K

Posted: Sun Jan 20, 2019 10:41 pm
by MadelineHlobik
Do you calculate Q the same way you calculate K? And then, you just compare Q to K to determine if more reactants are produced or not?

Re: Q VS. K

Posted: Sun Jan 20, 2019 10:43 pm
by mahika_nayak_3L
Yes, Q and K are calculated in the same way. Q is compared to K to determine which way the reaction will shift. If Q < K then then the forward reaction is favored and if Q > K then the reverse reaction is favored.

Re: Q VS. K

Posted: Sun Jan 20, 2019 10:50 pm
by 404975170
Q changes as the reaction of the system approaches equilibrium versus K that is the numerical value of Q at the "end" of the reaction, when equilibrium is reached. They are the same calculation but different significances.

Re: Q VS. K

Posted: Sun Jan 20, 2019 10:56 pm
by Simran Rai 4E
K is basically the Q, but at equilibrium.

Re: Q VS. K

Posted: Thu Jan 24, 2019 10:26 am
by Stevin1H
Q is calculated the same was as K with products/reactants, but Q is the value not at equilibrium. In respect to the equilibrium constant K, if Q<K, this means the concentration of reactants is greater than the concentration of products, so forward reaction is favored to reach equilibrium. If Q>K, this means the concentration of products is greater than the concentration of reactants so reverse reaction is favored.

Re: Q VS. K

Posted: Thu Jan 24, 2019 10:14 pm
by Jennifer Torres 2L
k is at equilibrium, Q is non equilibrium you use an ice table to solve for both.

Re: Q VS. K

Posted: Sat Jan 26, 2019 8:11 pm
by Vana Mirzakhani 3I
Yes, both are solved in the same way. Once both values are found, compare both to see if Q=K, which means the solution is at equilibrium.

Re: Q VS. K

Posted: Wed Jan 30, 2019 10:29 pm
by Krista Mercado 1B
Q and K are calculated the same way. If Q<K, then the reaction will tend to proceed towards the products. If Q>K, then the reaction will proceed towards the reactants.

Re: Q VS. K

Posted: Mon Feb 18, 2019 2:22 am
by Hadji Yono-Cruz 2L
Q and K are calculated in the same way. Q is calculated at any point of the reaction, but K is calculated only at equilibrium. If Q is less than K then the products are favored. If Q is less than K then the reactants are favored.

Re: Q VS. K

Posted: Mon Feb 18, 2019 9:47 pm
by Lauren Huang 1H
Both can be calculated the same way. The only difference is that Q is when the reaction is not at equilibrium and K is when the reaction is at equilibrium.

Re: Q VS. K

Posted: Sat Mar 16, 2019 8:36 am
by Nikki Bych 1I
Yes! Q is just when the reaction is not at equilibrium, but is calculated the same way.

Re: Q VS. K

Posted: Sat Mar 16, 2019 7:26 pm
by 404975170
When Q>K think of drawing a little pac man guy off the greater than sign and his mouth is going towards the reactants so the reaction favors reactants and if Q<K draw the pac man going towards the products side so the reaction favors the formation of products. Silly tip but useful.

Re: Q VS. K

Posted: Sat Mar 16, 2019 7:52 pm
by CristinaMorales1F
what is the difference between Q and K? if there a difference in the time it is calculated in terms of reaching equilibrium?

Re: Q VS. K

Posted: Sat Mar 16, 2019 9:07 pm
by Subhani Diu 1F
K is the reaction at equilibrium and Q is used to calculate the ratio at anytime, but they are both calculated the same way. If Q<K then the reactants are favored and will shift towards the products (forward. If Q>K then the products are favored and will shift towards the reactants (reverse).