Chemistry

Chemistry

Problem

The equilibrium constant for the reaction N2+3H2⇌2NH3\text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3 has a value of 7.76×10−57.76 \times 10^{-5} at 700 K. What does this value suggest about the position of the equilibrium at this temperature?
Intuitive explanation

A very small equilibrium constant means the reaction barely proceeds forward—the denominator (reactants) in the KcK_c expression vastly outweighs the numerator (products). At 700 K, this system strongly favors the reactants, so you'd expect to find mostly N2\text{N}_2 and H2\text{H}_2 remaining, with very little NH3\text{NH}_3 formed. This is why industrial ammonia synthesis requires lower temperatures and high pressures to shift the balance toward products.

Intuitive explanation

A very small equilibrium constant means the reaction barely proceeds forward—the denominator (reactants) in the KcK_c expression vastly outweighs the numerator (products). At 700 K, this system strongly favors the reactants, so you'd expect to find mostly N2\text{N}_2 and H2\text{H}_2 remaining, with very little NH3\text{NH}_3 formed. This is why industrial ammonia synthesis requires lower temperatures and high pressures to shift the balance toward products.

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