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# why can you use equilibrium moles to work out kc rather than concentrations???? watch

1. why can you use equilibrium moles to work out kc rather than concentrations????

for example using this simple equation:

1A+1B <----> 1C + 1D
2. Because its a ratio of things, when you put them into the equation for Kc, the fraction will have the same value whether you use concentrations or moles. The ratio of the concentrations of the reagents will be the same as the ratio of the moles at equilibrium. I explained that badly, but you might get some information out of it.
3. (Original post by The Randy Panda)
Because its a ratio of things, when you put them into the equation for Kc, the fraction will have the same value whether you use concentrations or moles. The ratio of the concentrations of the reagents will be the same as the ratio of the moles at equilibrium. I explained that badly, but you might get some information out of it.
yeah i get what you mean but why equilibrium moles rather than concentration, if they going to give the same ratio?
4. You might only be able to use moles. Or, you might have moles, but can't be bothered to convert them into concentration. Chemists are as lazy as possible :P

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