A combustion reaction of a hydrocarbon is defined as thereaction of the compound into carbon dioxide and water.
CmHn(g) + (m+(1/4)n)O2(g) ---> mCO2 + (1/2)nH2O(l)
1. Demonstrate that this chemical reaction is balanced.
2a. From this definition, write down the chemical reaction forthe combustion of cyclopropane, C3H6(g).
2b. The enthalpy of reaction for the combustion of cyclopropane(i.e., the reaction in 2a) is measured to be ΔH° rxn = −2091 kJ/molin the standard state at 25° C. Find the standard state enthalpy offormation, ΔH° f , at 25° C for CO2(g) and H2O(l) in a chemistrytextbook. Use this information to determine the enthalpy offormation for cyclopropane in the standard state at 25° C.
2c. Propene is an isomer of cyclopropane. At 1bar pressure and atemperature of 25° C, the enthalpy of formation for propene is+20.42 kJ mol-1 . Determine the enthalpy of reaction for theisomerization reaction:
cyclopropane (g) → propene (g) ,
at 1bar pressure and a temperature of 25° C.
