Melting and Boiling

Part of the Energy, Rates and Equilibrium section of Coddy's Chemistry journey. Lesson 12 of 35.

On a flat step the energy pulls the particles apart; the temperature stands still.

Water: melting $6.0\ \mathrm{kJ/mol}$ , boiling $40.7\ \mathrm{kJ/mol}$ . Boiling separates the particles completely, so it takes far more.

$q = n \times \Delta H \qquad n = \frac{m}{M}$

Freezing and condensing give the same energy out.

Challenge

An ice cube of $36\ \mathrm{g}$ melts in a drink. Water is $18\ \mathrm{g/mol}$ and melting takes $6.0\ \mathrm{kJ/mol}$ . How much energy $q$ does the ice take from the drink?

Try it yourself

Solve for $q$

Test yourself

This lesson includes a short quiz. Start the lesson to answer it and track your progress.

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 Plant Recap - 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 CurvesMelting and BoilingEnergy 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