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Standard Enthalpy of Formation

Chemistry ⇒ Thermochemistry and Energetics

Standard Enthalpy of Formation starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Standard Enthalpy of Formation. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 11
Calculate the standard enthalpy change for the reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH−f° [CO(g)] = -110 kJ/mol and ΔH−f° [CO2(g)] = -394 kJ/mol.
Describe how standard enthalpy of formation values are used to calculate the enthalpy change of a chemical reaction.
Describe the difference between standard enthalpy of formation and standard enthalpy of combustion.
Describe the importance of standard enthalpy of formation values in calculating enthalpy changes for chemical reactions.
Explain why the standard enthalpy of formation of Cl2(g) is zero.
Explain why the standard enthalpy of formation of diamond is not zero.
Explain why the standard enthalpy of formation of F2(g) is zero.
Explain why the standard enthalpy of formation of H2O(g) is different from that of H2O(l).
Given the following data: ΔH−f° [C2H5OH(l)] = -277 kJ/mol, ΔH−f° [CO2(g)] = -394 kJ/mol, ΔH−f° [H2O(l)] = -286 kJ/mol. Calculate the enthalpy change for the reaction: C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l).
Given the following data: ΔH−f° [C6H12O6(s)] = -1273 kJ/mol, ΔH−f° [CO2(g)] = -394 kJ/mol, ΔH−f° [H2O(l)] = -286 kJ/mol. Calculate the enthalpy change for the reaction: C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l).
Given the following data: ΔH−f° [CH4(g)] = -75 kJ/mol, ΔH−f° [CO2(g)] = -394 kJ/mol, ΔH−f° [H2O(l)] = -286 kJ/mol. Calculate the enthalpy change for the reaction: CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l).
Given the following data: ΔH−f° [NaCl(s)] = -411 kJ/mol, ΔH−f° [Na(s)] = 0, ΔH−f° [Cl2(g)] = 0. Calculate the enthalpy change for the reaction: 2 Na(s) + Cl2(g) → 2 NaCl(s).
Given the following data: ΔH−f° [NH3(g)] = -46 kJ/mol, ΔH−f° [N2(g)] = 0, ΔH−f° [H2(g)] = 0. Calculate the enthalpy change for the reaction: N2(g) + 3 H2(g) → 2 NH3(g).
Given the following standard enthalpies of formation: ΔH−f° [NO2(g)] = 34 kJ/mol, ΔH−f° [NO(g)] = 90 kJ/mol, calculate the enthalpy change for the reaction: 2 NO(g) + O2(g) → 2 NO2(g).
If the standard enthalpy of formation of NH3(g) is -46 kJ/mol, what does the negative sign indicate?
State Hess's Law and explain its relevance to standard enthalpy of formation.
State the standard conditions under which standard enthalpy of formation is measured.
The standard enthalpy of formation of C2H6(g) is -84.7 kJ/mol. Write the formation equation for C2H6(g).
Write the balanced chemical equation for the standard enthalpy of formation of CO2(g).