This question is about the equilibrium:
N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g})N2(g)+3H2(g)⇌2NH3(g)
State and explain the effect, if any, of an increase in overall pressure on the equilibrium yield of NH3\text{NH}_3NH3.
A 0.500 mol0.500\text{ mol}0.500 mol sample of N2\text{N}_2N2 is mixed with a 1.200 mol1.200\text{ mol}1.200 mol sample of H2\text{H}_2H2 in a sealed container at a constant temperature. When equilibrium is reached at a total pressure of 250 kPa250\text{ kPa}250 kPa, the mixture contains 0.300 mol0.300\text{ mol}0.300 mol of NH3\text{NH}_3NH3.
Calculate the partial pressure, in kPa\text{kPa}kPa, of N2\text{N}_2N2 in this equilibrium mixture.
A different mixture of N2\text{N}_2N2 and H2\text{H}_2H2 reaches equilibrium at a different temperature. The table below shows the partial pressures of the gases at equilibrium:
| Gas | Partial pressure / kPa\text{kPa}kPa |
|---|---|
| N2\text{N}_2N2 | 2.00×1022.00 \times 10^22.00×102 |
| H2\text{H}_2H2 | 1.50×1021.50 \times 10^21.50×102 |
| NH3\text{NH}_3NH3 | 4.50×1014.50 \times 10^14.50×101 |
Give an expression for the equilibrium constant (KpK_pKp) for this reaction. Calculate the value of the equilibrium constant for this reaction and give its units.
What is the effect on the value of KpK_pKp if the pressure of this equilibrium mixture is increased at a constant temperature?
Select one option: