5. Calculate the enthalpy of formation of hexane (CsH4 ()) at 25 °C, given that the...
Calculate the standard combustion enthalpy of propylene at 25 ° C using the standard formation enthalpy of liquid water (-286 kJ mol-1) and the following reactions: 1) CH2CHCH3 (g) + H2 (g) → CH3CH2CH3 (g); Δ? (1) = -125 kJ mol-1 2) CH3CH2CH3 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l); Δ? (2) = -2220 kJ mol-1 3) H 2 (g) + 0.5O2 (g) → H2O (l);Δ? ((3) = -286 kJ mol-1
Hexane is a common laboratory solvent and a component of petrol. Its combustion reaction is as follows: 2 C6H14 (g) + 19 O2(g) ⟶ 12 CO2(g) + 14 H2O(l) Δ rHo = -8326 kJ mol-1 Use the reaction enthalpy value to calculate the heat in (kJ mol-1) released by combustion of 0.138 mol of hexane.
Calculate the AH formation of octane, CBH1B (), given that the enthalpy of combustion of octane is -5471 kl/mol and the standard enthalpies of formation of H20 () and CO2 (g) are -393.5 kJ/mol and -285.8 kJ/mol respectively.
The combustion of hexane is given by the following reaction. 2 C6H14 + 19 O2 12 CO2 + 14 H2O The enthalpy of reaction is −4163.0 kJ/mol. How much energy (in joules) will be released if 82.22 grams of hexane is burned. (Molar mass of hexane = 86.20 g/mol). J
4. (a) Calculate the Gibbs Free Energy of formation for urea at 25°C. Given: The standard enthalpy of formation is -333.17 kJ mol and the standard entropy of formation is 136.093 J K mol". (b) is the formation of urea a spontaneous process under these conditions? Explain. (7 pts) J mol
The standard molar enthalpy of formation of sucrose (C12H22O11) is -2222 kJ/mol. What is the enthalpy of combustion of a sugar cube of sucrose weighing 2 g? If 25% of this energy can be converted to work by the human body, to what height can a 100 kg man climb on the energy derived from such a sugar cube? Assume the man is on the surface of the Earth.
Be sure to answer all parts. At 25°C, the standard enthalpy of formation of HF(aq) is -320.1 kJ/mol. Of OH(aq), it is -229.5 kJ/mol. Of F (aq), it is -330.2 kJ/mol, and of H2O(l), it is -285.9 kJ/mol. (a) Calculate the standard enthalpy of neutralization of HF(aq): HF(aq) + OH(aq) + (aq) + H2O(1) kJ/mol (b) Using the value of -56.3 kJ as the standard enthalpy change for the reaction H(aq) + OH(aq) +H2O(1) calculate the standard enthalpy of change...
The standard enthalpy of combustion of cyclopropane is -2091 kJ/mol at 298 K. The enthalpy of formation of CO_2 (g) and H_2 O (I) are -393 kJ/mol and -286 kJ/mol, respectively. Calculate the enthalpy of formation of cyclopropane Given that the enthalpy of formation of propene is 20.42 kJ/mol, please calculate the enthalpy of isomerization of cyclopropane to propene.
3. The standard enthalpy of formation of ethylbenzene (C3H10 (1)] is -12.5 kJ mol!. Calculate its standard enthalpy of combustion. (AH®(CO2 (g)) = -393.51kJ mol', AH®, (H20 (1))= -285.83 kJ mol'). (Note: to solve this question you should write the balanced equation of ethylbenzene combustion reaction)
7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s) + O2(g) + CO2(g) b. S(s) + O2(g) → SO2(e) C. CS2() + 302(g) → CO2(g) + ' 250 (6) AH° = -393.5 kJ/mol AH° = -296.4 kJ/mol AH° = -1073.6 kj/mol (the standard state of the element Sulfur is S(s))