Menu

Recap - Methanol Plant

Part of the Energy, Rates and Equilibrium section of Coddy's Chemistry journey. Lesson 33 of 35.

Challenge

Methanol is a fuel and a raw material for plastics. Factories make it from carbon monoxide and hydrogen over a copper catalyst, at about $250\ \mathrm{^{\circ}C}$ and $50\ \mathrm{atm}$ :

$\mathrm{CO(g)} + 2\mathrm{H_2(g)} \rightleftharpoons \mathrm{CH_3OH(g)} \qquad \Delta H = -90\ \mathrm{kJ}$

An engineer suggests running the reactor at $350\ \mathrm{^{\circ}C}$ to make it faster. At the higher temperature, which way does the equilibrium shift, and what happens to K?

Try it yourself

EquilibriumWhich way does it shift?

CO(g)2 H₂(g)CH₃OH(g)

All lessons in Energy, Rates and Equilibrium

1Energy in Reactions

Exothermic and Endothermic Energy Diagrams Enthalpy Change Activation Energy Recap - Hand Warmer

4Rates of Reaction

Collision Theory Concentration and Rate Temperature and Rate Surface Area Catalysts Recap - Speed Trials

7Practice Problems

Recap - Methanol PlantRecap - Butane Lighter Recap - Limestone Kiln

2Bond Energies

Breaking and Making Bonds Delta H from Bond Energies Hess's Law Energy and Moles Recap - Fuel Value

5Equilibrium

Reversible Reactions Dynamic Equilibrium The Equilibrium Constant Writing K Solids and Liquids in K Recap - K Builder

3Changes of State

Heating Curves Melting and Boiling Energy of State Changes Recap - Ice to Steam

6Changing an Equilibrium

Le Chatelier's Principle Changing Concentration Changing Pressure Changing Temperature The Haber Process Recap - Factory Settings