Recap - Butane Lighter

Part of the Energy, Rates and Equilibrium section of Coddy's Chemistry journey. Lesson 34 of 35.

Challenge

A pocket lighter holds liquid butane, C₄H₁₀ ( $58\ \mathrm{g/mol}$ ), under pressure. When it is lit, butane gas burns:

$2\mathrm{C_4H_{10}} + 13\mathrm{O_2} \rightarrow 8\mathrm{CO_2} + 10\mathrm{H_2O}$

Burning one mole of butane has $\Delta H = -2877\ \mathrm{kJ/mol}$ . A student weighs the lighter before and after heating a beaker of water, and finds it has lost $2.9\ \mathrm{g}$ . What is the heat change $Q$ of the butane that burned?

Try it yourself

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 PlantRecap - Butane LighterRecap - 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