Question

THERMODYNAMICS (ASSIGNMENT
1) Calculate the C=C bond energy in ethene:
H2C=CH2(g) + Ha(g) -> H3C-CH3(g) ∆H = -138 kJ/mol
Bond enthalpies (kJ/mol): C-C = 348; H-H = 436; C-H = 412
2) Calculate the standard enthalpy of formation of one mole of CH3OH (1), if
the combustion of one mole of methanol takes place at 298 K and 1 atm and
after combustion CO2 (g) and H20 (1) are produced and -726 kJ of heat is
liberated. Assume that the standard enthalpies of formation of CO2 (g) and
H20 (1) are - 393 kJ/mol and -286 kJ/mol respectively.
3) The combustion of one mole of methane takes place at 298 K and 1 atm.
After combustion, CO2(g) and H20 (1) are produced and 890.0 kJ of heat is
liberated. Calculate the standard enthalpy of formation of methane. Standard
enthalpies of formation of CO2(g) and H.O(l) are -393.5 kJ mol-1 and -285.83
kJ mol respectively,
4) Enthalpies o, formation of CO (g), CO2(g), N2O(g) & N204(g) are -110,-- 393.
81 & 3.7 kJ molt respectively. Find the value of enthalpy for the reaction:
N204 (g) + 3C0(g) ->N2O(g) + 3CO2(g)​

Answer 1

Answer:t

Explanation: