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Topic: AP Chemistry Equilibrium Problem  (Read 13832 times)

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Offline FoolishChild

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AP Chemistry Equilibrium Problem
« on: March 05, 2010, 10:59:29 PM »
I need help on this question:

"The equilibrium concentration of FeSCN2+ ions in each reference solution listed below is essentially equal to the concentration of SCN- ions in solution before any reaction occurs." Use Le Chatlier's Principle to explain why this statement is true.

I don't understand why the statement is true, even though I know what Le Chatlier's Principle states.

Offline Borek

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Re: AP Chemistry Equilibrium Problem
« Reply #1 on: March 06, 2010, 03:43:51 AM »
I would say it is a simple stoichiometry, no need for LeChatelier's principle. Equilibrium constant for the reaction is high enough.
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Offline FoolishChild

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Re: AP Chemistry Equilibrium Problem
« Reply #2 on: March 06, 2010, 12:26:35 PM »
I would say it is a simple stoichiometry, no need for LeChatelier's principle. Equilibrium constant for the reaction is high enough.

Here is some of the stuff I had left out, the table:


Offline Borek

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Re: AP Chemistry Equilibrium Problem
« Reply #3 on: March 06, 2010, 02:02:20 PM »
I see what they mean. Compare concentrations.
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Offline FoolishChild

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Re: AP Chemistry Equilibrium Problem
« Reply #4 on: March 06, 2010, 03:21:17 PM »
I see what they mean. Compare concentrations.

The concentration of Fe is higher than concentration of SCN. How do I explain how the stateman is true though? It's talking about Keq, and I don't know what the equilibrium reaction is and how to input Le Chatlier's principle into the statement.

Offline Borek

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Re: AP Chemistry Equilibrium Problem
« Reply #5 on: March 06, 2010, 04:38:37 PM »
What is the reaction between Fe3+ and SCN-?
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