Science, Tech, Math › Science Enthalpy Change Example Problem Enthalpy Change of the Decomposition of Hydrogen Peroxide Share Flipboard Email Print PM Images/Getty Images Science Chemistry Basics Chemical Laws Molecules Periodic Table Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Anne Marie Helmenstine, Ph.D. Chemistry Expert Ph.D., Biomedical Sciences, University of Tennessee at Knoxville B.A., Physics and Mathematics, Hastings College Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels. our editorial process Facebook Facebook Twitter Twitter Anne Marie Helmenstine, Ph.D. Updated December 26, 2018 This example problem shows how to find the enthalpy for the decomposition of hydrogen peroxide. Enthalpy Review You may wish to review the Laws of Thermochemistry and Endothermic and Exothermic Reactions before you begin. Enthalpy is a thermodynamic property that is the sum of the internal energy that is added to a system and the product of its pressure and volume. It's a measure of the system's capacity to release heat and perform non-mechanical work. In equations, enthalpy is denoted by the capital letter H, while specific enthalpy is lowercase h. Its units are usually joules, calories, or BTUs. The change in enthalpy is directly proportional to the number of reactants and products, so you work this type of problem using the change in enthalpy for the reaction or by calculating it from the heats of formation of the reactants and products and then multiplying this value times the actual quantity (in moles) of material that is present. Enthalpy Problem Hydrogen peroxide decomposes according to the following thermochemical reaction:H2O2(l) → H2O(l) + 1/2 O2(g); ΔH = -98.2 kJCalculate the change in enthalpy, ΔH, when 1.00 g of hydrogen peroxide decomposes. Solution This sort of problem is solved by using a table to look up the change in enthalpy unless it's given to you (as it is here). The thermochemical equation tells us that ΔH for the decomposition of 1 mole of H2O2 is -98.2 kJ, so this relationship can be used as a conversion factor. Once you know the change in enthalpy, you need to know the number of moles of the relevant compound to calculate the answer. Using the Periodic Table to add up the masses of hydrogen and oxygen atoms in hydrogen peroxide, you find the molecular mass of H2O2 is 34.0 (2 x 1 for hydrogen + 2 x 16 for oxygen), which means that 1 mol H2O2 = 34.0 g H2O2. Using these values: ΔH = 1.00 g H2O2 x 1 mol H2O2 / 34.0 g H2O2 x -98.2 kJ / 1 mol H2O2ΔH = -2.89 kJ Answer The change in enthalpy, ΔH, when 1.00 g of hydrogen peroxide decomposes = -2.89 kJ It's a good idea to check your work to make sure the conversion factors all cancel out to leave you with an answer in energy units. The most common error made in the calculation is accidentally switching the numerator and denominator of a conversion factor. The other pitfall is significant figures. In this problem, the change in enthalpy and mass of sample both were given using 3 significant figures, so the answer should be reported using the same number of digits.