A company makes hydrogen chloride, HCl\text{HCl}HCl, gas by reacting hydrogen gas with chlorine gas.
Look at the equation for the reaction: H2(g)+Cl2(g)⇌2HCl(g)\text{H}_2(\text{g}) + \text{Cl}_2(\text{g}) \rightleftharpoons 2\text{HCl}(\text{g})H2(g)+Cl2(g)⇌2HCl(g)
What is the volume of hydrogen gas, in dm3\text{dm}^3dm3, needed to react with 480 dm3480\text{ dm}^3480 dm3 chlorine at room temperature and pressure? Use the balanced symbol equation to help you.
Calculate the volume of hydrogen chloride formed, in dm3\text{dm}^3dm3, when 480 dm3480\text{ dm}^3480 dm3 of chlorine completely reacts with hydrogen at room temperature and pressure. Use the balanced symbol equation to help you.
Calculate the mass, in kilograms, of 480 dm3480\text{ dm}^3480 dm3 of chlorine at room temperature and pressure.
One mole of any gas occupies 24 dm324\text{ dm}^324 dm3.
Give your answer to 1 decimal place.
(The relative molecular mass, MrM_rMr, of Cl2\text{Cl}_2Cl2 is 71.071.071.0).
The reaction to make hydrogen chloride is an equilibrium reaction: H2(g)+Cl2(g)⇌2HCl(g)\text{H}_2(\text{g}) + \text{Cl}_2(\text{g}) \rightleftharpoons 2\text{HCl}(\text{g})H2(g)+Cl2(g)⇌2HCl(g)
The forward reaction is exothermic.
The yield of hydrogen chloride and the rate at which the reaction reaches equilibrium are affected by different conditions.
Look at two possible reaction conditions, C and D, the company could use for this reaction.
| Temperature (∘C^\circ\text{C}∘C) | Pressure (atmospheres) | Catalyst? | |
|---|---|---|---|
| C | 350 | 1 | Yes |
| D | 600 | 4 | No |
The company decides to use reaction conditions C, instead of D.
Explain why they make this choice. Use ideas about rate of reaction and position of equilibrium to help you.