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Consider the reaction of nitrogen gas with hydrogen gas to make ammonia gas at equilibrium in a closed container with a piston at $300 °C$. The piston can move freely. The equilibrium constant, $K_p$, for this reaction is $4.3 \times 10^{-3}$.

Which of the following will change the equilibrium constant?

Select ALL that apply.


Increasing the temperature.


Increasing the pressure.


Adding reactants to the container.


Adding nonreactive argon gas to the container.

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