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# What does it mean when the equilibrium shifts to the right Watch

1. the pressure increases so the equilibrium shifts to the right

The mark scheme says that NO2 concentration increases more than N2O4. I'm confused

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2. there's the actual question and me writing in the correct answers

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3. Are you familiar with Le Chatelier's principle?

If you increase the overall pressure of the equilibrium, the system moves to decrease the overall pressure - in this instance by producing less moles of gas (since an ideal gas has a fixed volume at a given temperature).

Equilibrium constants are only affected by changes in temperature.
4. Have a read of this:

http://www.chemguide.co.uk/physical/...chatelier.html
5. (Original post by EierVonSatan)
Are you familiar with Le Chatelier's principle?

If you increase the overall pressure of the equilibrium, the system moves to decrease the overall pressure - in this instance by producing less moles of gas (since an ideal gas has a fixed volume at a given temperature).

Equilibrium constants are only affected by changes in temperature.
But why does NO2 increase? there's more moles of NO2 then there is of N2O4

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6. (Original post by rambo1168)
But why does NO2 increase? there's more moles of NO2 then there is of N2O4
It helps to stick some imaginary numbers in. Say that Kc = 4 and that [NO2] = 1 and [N2O4] = 4 to start with:

The concentration's double briefly, meaning that the [NO2]2 increases more than [N2O4, and the fraction becomes more bottom heavy (smaller):

Now the equilibrium shifts to restore the original value of 4 (or close enough ) by converting 2NO2 into N2O4:

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