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Recap - Ice to Steam

Part of the Energy, Rates and Equilibrium section of Coddy's Chemistry journey. Lesson 14 of 35.

Challenge

A camper melts $18\ \mathrm{g}$ of ice ( $1\ \mathrm{mol}$ ) at $273\ \mathrm{K}$ , warms the water to $373\ \mathrm{K}$ and boils it all away. Melting takes $6.0\ \mathrm{kJ/mol}$ , boiling $40.7\ \mathrm{kJ/mol}$ , and water's specific heat is $4.18\ \mathrm{J/(g·K)}$ . How much energy $Q$ , in kJ, does the stove give?

Try it yourself

Physics diagram: beaker

Solve for $Q$

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 Curves Melting and Boiling Energy of State ChangesRecap - Ice to Steam

6Changing an Equilibrium

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