Q and K

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Q and K

Postby Dakota_Campbell_1C » Thu Jan 10, 2019 9:44 pm

If K is the equilibrium constant, or the rate at which both the forward and reverse reaction are happening simultaneously. What is the Q value and what is its significance in determining whether the products or the reactants are going to be favoured?

Parth Mungra
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Re: Q and K

Postby Parth Mungra » Thu Jan 10, 2019 9:48 pm

Q is the reaction quotient, and this determines which direction a reaction will proceed during a given moment. You can calculate Q by taking the concentration of the products over the concentration of the reactants. If Q>K then forward reaction is favored and more reactants. If Q<K, then the reverse reaction is favored and more products

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Re: Q and K

Postby Schuyler_Howell_4D » Thu Jan 10, 2019 10:12 pm

Can you clarify please because if you calculate Q the same way you calculate K how can they be different values?

Lumbini Chandrasekera 1B
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Re: Q and K

Postby Lumbini Chandrasekera 1B » Thu Jan 10, 2019 11:52 pm

Q and K are different values because when you're given the problem, it is not explicitly stated whether the reaction is at equilibrium at the moment. You have to determine this by using the K formula and plugging in the concentration values to determine what state the reaction is in by comparing it to the correct K value.

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Re: Q and K

Postby Andre_Galenchik_2L » Fri Jan 11, 2019 12:32 am

Basically in a question you are given the K value of the reaction when it is at equilibrium. The reaction that you have to work with is not at equilibrium so by finding the reaction quotient, you can figure out which way the reaction will be favored.

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