An industrial plant synthesizes hydrogen fluoride, HF\text{HF}HF, gas by reacting hydrogen gas with fluorine gas.
Look at the equation for this reversible reaction: H2(g)+F2(g)⇌2HF(g)\text{H}_2(\text{g}) + \text{F}_2(\text{g}) \rightleftharpoons 2\text{HF}(\text{g})H2(g)+F2(g)⇌2HF(g)
What is the volume of hydrogen gas, in dm3\text{dm}^3dm3, needed to react completely with 912 dm3912\text{ dm}^3912 dm3 of fluorine at room temperature and pressure? Use the balanced symbol equation to help you.
Calculate the volume of hydrogen fluoride formed, in dm3\text{dm}^3dm3, when 912 dm3912\text{ dm}^3912 dm3 of fluorine completely reacts with hydrogen at room temperature and pressure. Use the balanced symbol equation to help you.
Calculate the mass, in kilograms, of 912 dm3912\text{ dm}^3912 dm3 of fluorine 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 F2\text{F}_2F2 is 38.038.038.0).
The reaction to make hydrogen fluoride is an equilibrium reaction: H2(g)+F2(g)⇌2HF(g)\text{H}_2(\text{g}) + \text{F}_2(\text{g}) \rightleftharpoons 2\text{HF}(\text{g})H2(g)+F2(g)⇌2HF(g)
The forward reaction is exothermic.
The yield of hydrogen fluoride and the rate at which the reaction reaches equilibrium are affected by different conditions.
Look at two possible reaction conditions, A and B, the plant could use for this reaction.
| Temperature (∘C^\circ\text{C}∘C) | Pressure (atmospheres) | Catalyst? | |
|---|---|---|---|
| A | 250 | 2 | Yes |
| B | 500 | 8 | No |
The company decides to use reaction conditions A, instead of B.
Explain why they make this choice. Use ideas about rate of reaction and position of equilibrium to help you.