Describe the changes in equilibrium of ethanol production from ethene and water (enthalpy of reaction is ∆H = - 46 kJ/mol) when: (a) a high pressure is applied; (b) ethanol concentration is increased; (c) temperature is increased; (d) a catalyst is used.

The equation for the reaction (would be given for this type of question but I ran out of space): C2H4 (g) + H2O (g) ⇌ C2H5OH (g) ∆H = - 46 kJ/molQuestion is based on Le Chatelier's principle: if a system in dynamic equilibrium is exposed to a change, processes will occur to oppose that change.Answers: (a) High pressure applied: the equilibrium will shift to the direction where less gas molecules are produced - to the right. That is because we have 2 mol of gases (ethene and water) on the left and only 1 mol on the right. (b) Ethanol concentration increased: the equilibrium will shift to the left, so that production of ethanol is reduced. (c) Temperature increased: the reaction that occurs left to right is exothermic (negative ∆H) - heat is released. Hence the equilibrium will shift in the opposite direction, as the reaction that occurs right to left is then endothermic (absorbs heat) and therefore will oppose the increase in temperature, so the equilibrium will shift to the left. (d) Catalyst used: no change in the position of equilibrium! (common trick question)

AA
Answered by Aiste A. Chemistry tutor

6769 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Devise a simple synthetic route to an amide from a carboxylic acid. Give a mechanism for the final step and explain why the reagents are not added 1:1 in the final step


What is the trend in reactivity of Group 2 elements with halogens as the group is descended?


Why does magnesium have a higher melting point than sodium?


What is hybridisation and how can it be used to explain the shapes of molecules?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences