Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C4H4 (–2341 kJ/ mol), C4H8 (–2755 kJ/ mol), and H2 (–286 kJ/ mol), calculate ΔH for the reaction C4H4(g) + 2H2(g) → C4H8(g)
Answer to relevant QuestionsGiven the following data: 2O3(g) → 3O2(g) ΔH = –427 kJ O2(g) → 2O(g) ΔH = 495 kJ NO(g) + O3(g) → NO2(g) + O2(g) ΔH = –199 kJ Calculate ΔH for the reaction NO(g) + O(g) → NO2(g) The combustion of methane can be represented as follows: a. Use the information given above to determine the value of ΔH for the combustion of methane to form CO2(g) and 2H2O(l). b. What is ΔHof for an element in its ...At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/ mol and 49 kJ/ mol, respectively. a. Calculate ΔHo for C6H6(l) → 3C2H2(g) b. Both acetylene (C2H2) and benzene (C6H6) can be used as ...Ethanol (C2H5OH) has been proposed as an alternative fuel. Calculate the standard enthalpy of combustion per gram of liquid ethanol. The bomb calorimeter in Exercise 87 is filled with 987 g of water. The initial temperature of the calorimeter contents is 23.32oC. A 1.056-g sample of benzoic acid (ΔEcomb = 226.42 kJ/ g) is combusted in the calorimeter. ...
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