Methanol (CH3OH) is often used as a fuel in high-performance engines in race cars. Using the data in the following table compare the standard enthalpy of combustion per gram of methanol with the enthalpy of combustion per gram of gasoline. Gasoline is actually a mixture of compounds, but assume for this problem that gasoline is pure liquid octane (C8H18).

A scientist measures the standard enthalpy change for the following reaction to be -737.2 kJ : 2Co(g) + 2 NO(g)2CO2(g) + N2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.

The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol

A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.

The balanced thermochemical equation for the combustion of exactly one mole of propane is: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O(l) ΔH = -2220 kJ/mol What is the enthalpy change for the reaction: 1.5 CO2 (g) + 2 H2O(l)  → 0.5 C3H8 (g) + 2.5 O2 (g) ΔH = ?

The combustion of 0.1556 g benzoic acid increases the temperature of a bomb calorimeter by 2.50°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C 8 A 0.2194-g sample of vanillin (Cg H8O3) is then burned in the same calorimeter, and the temperature increases by 3.20°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol

A scientist measures the standard enthalpy change for the following reaction to be -912.5 kJ:2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is  kJ/mol.

3. Write a balanced chemical reaction for the synthesis of methane (CH4) and liquid water from hydrogen and acetic acid (CH3COOH) and calculate the standard enthalpy of the reaction by using the appropriate enthalpies of formation on page 308 or Appendix 4 in the textbook.

Using the standard enthalpies of formation in the picture, calculate ΔHº for the following reactions:a) 2H2O2 (l) → 2H2O (l) + O2 (g) b) CH4 (g) + Cl2 (g) → CH3Cl (g) + HCl (g) c) HCl (g) + NaOH (s) → NaCl (s) + H2O (l)

A scientist measures the standard enthalpy change for the following reaction to be - 770.6 kJ: 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O (1) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(1) is kJ/mol. Substance AH (kJ/mol) NO(g) H₂(g) N₂ (9) 90.3 0.0 0.0