If we change the initial concentrations do the equilibrium concentrations change?

Now place 10 moles of N2 and 10 moles of H2 into the reaction vessel and press "equilibrate". Write down the number of moles of each substance that you have at equilibrium. Convert from number of moles to molarity.

Again plug the concentrations of N2, H2, and NH3 into the equilibrium constant expression. Verify that this expression gives the value of Kc that you expect.

If you change the starting concentrations of the reactants do the equilibrium concentrations of the species change? (Hint: compare the equilibrium concentrations when you put in 1 mole H2 and 1 mole N2 versus when you put in 10 moles of H2 and 10 moles of N2)
 
Yes, because the equilibrium concentrations of each species depend on the initial concentrations of each species.
No, we always get the same concentration of each species.
   

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