How the magnitude of "K"
affects the extent of reaction

Change the value of the equilibrium constant to 0.10 by changing the temperature on the thermometer. Place 3 moles of N2 and 3 moles of H2 into the reaction vessel. Press "equilibrate".

At equilibrium the number of moles of NH3 produced equals:
0 moles
0.48 moles
0.96 moles
It is impossible to know

Now change the value of "Kc" from 0.10 to 0.65. Again place 3 moles of N2 and 3 moles of H2 into the reaction vessel. Press "equilibrate".

At equilibrium the number of moles of NH3 produced equals:
0 moles
0.96 moles
1.30 moles
It is impossible to know


From the results of the last two questions we can conclude that as the magnitude of "K" increases:

There is no change in the concentration of product molecules compared to the concentration of reactant molecules at equilibrium.
The concentration of product molecules increases compared to the concentration of reactant molecules.
The concentration of reactant molecules increases compared to the concentration of product molecules.
The concentration of products and reacts increases by the same amount.

 

When would it reasonable to assume that all of the limiting reagent reacts and is converted into product molecules?
When the equilibrium constant is a very small number.
When the equilibrium constant is a very large number.
The limiting reagent is always completely used up.
There is always a significant amount of limiting reagent left at equilibrium.

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