Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is increased by adding an inert gas (and everything else is held constant)?N2(g) + 3H2(g) 2NH3(g)
Question
Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is increased by adding an inert gas (and everything else is held constant)?N2(g) + 3H2(g) 2NH3(g)
Solution
The addition of an inert gas at constant volume does not change the partial pressures of the individual gases in the system. Therefore, it does not affect the position of the equilibrium. So, for the given exothermic reaction, the equilibrium will not shift if the pressure is increased by adding an inert gas and everything else is held constant.
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