This question is about some gas mixtures at equilibrium.
This reaction can be used to produce hydrogen iodide:
H2(g)+I2(g)⇌2HI(g)ΔH=−9.4 kJ mol−1\text{H}_2(\text{g}) + \text{I}_2(\text{g}) \rightleftharpoons 2\text{HI}(\text{g}) \quad \Delta H = -9.4\text{ kJ mol}^{-1}H2(g)+I2(g)⇌2HI(g)ΔH=−9.4 kJ mol−1
A mixture of 2.50 mol2.50\text{ mol}2.50 mol of H2(g)\text{H}_2(\text{g})H2(g) and 2.50 mol2.50\text{ mol}2.50 mol of I2(g)\text{I}_2(\text{g})I2(g) is allowed to reach equilibrium at a constant temperature in a 10 dm310\text{ dm}^310 dm3 container.
At equilibrium, there are 3.60 mol3.60\text{ mol}3.60 mol of HI(g)\text{HI}(\text{g})HI(g).
Calculate the mole fraction of HI(g)\text{HI}(\text{g})HI(g) in the equilibrium mixture.
State why the equilibrium constant (KpK_{\text{p}}Kp) for this reaction has no units.
The temperature of the equilibrium mixture is increased. How does the amount of HI(g)\text{HI}(\text{g})HI(g) change when the new position of equilibrium is reached? Select one:
Phosgene can be synthesized from carbon monoxide and chlorine:
CO(g)+Cl2(g)⇌COCl2(g)ΔH=−108 kJ mol−1\text{CO}(\text{g}) + \text{Cl}_2(\text{g}) \rightleftharpoons \text{COCl}_2(\text{g}) \quad \Delta H = -108\text{ kJ mol}^{-1}CO(g)+Cl2(g)⇌COCl2(g)ΔH=−108 kJ mol−1
The table below shows the mole fractions of each gas in an equilibrium mixture at a total pressure of 4000 kPa4000\text{ kPa}4000 kPa.
| Gas | Mole fraction |
|---|---|
| Carbon monoxide, CO\text{CO}CO | 0.5200.5200.520 |
| Chlorine, Cl2\text{Cl}_2Cl2 | 0.4100.4100.410 |
| Phosgene, COCl2\text{COCl}_2COCl2 | 0.07000.07000.0700 |
Give an expression for KpK_{\text{p}}Kp for this reaction.
Calculate the value of KpK_{\text{p}}Kp at 4000 kPa4000\text{ kPa}4000 kPa. State the units.
State the effect, if any, of an increase in the volume of the container on the value of KpK_{\text{p}}Kp for this reaction at a constant temperature.