From the Post-Module Assessment 1A:

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Miguel Velasco 2J
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From the Post-Module Assessment 1A:

Postby Miguel Velasco 2J » Wed Nov 29, 2017 11:09 pm

what is the difference between when a reaction is said to "Lie to the right " vs when the “equilibrium is shifted to the right” vs with respect to equilibrium constants?
Last edited by Miguel Velasco 2J on Wed Nov 29, 2017 11:28 pm, edited 1 time in total.

Jean Mok 3K
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Re: From the Post-Module Assessment 1A:

Postby Jean Mok 3K » Wed Nov 29, 2017 11:26 pm

To be honest I am not too sure about this exactly but from my understanding there is not much of a difference between the first two things that you quoted. I am not exactly sure about the third.

Aijun Zhang 1D
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Re: From the Post-Module Assessment 1A:

Postby Aijun Zhang 1D » Wed Nov 29, 2017 11:28 pm

"Lie to the right" is used when describing K at the equilibrium. It is a state.
From the note, if K is small (K<10^-3), more reactants are at equilibrium. So the equilibrium sits to the left. Vice versa.
This basically describes which side is favored.

While "equilibrium shifts to the right" describes a dynamic situation. For a reaction, if more reactants are added, the concentration of reactants increases. So the equilibrium will shift to products (assuming products are on right side) to compensate the excess reactants, to minimize the effect of changes. This is more about change in concentration, pressure and temperature causing changes in the equilibrium shifts. The Kc is not changed during this process under the same temperature.

Miguel Velasco 2J
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Re: From the Post-Module Assessment 1A:

Postby Miguel Velasco 2J » Wed Nov 29, 2017 11:34 pm

Makes sense thank you!


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