Calculate ΔHo for C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l)
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ΔHof C6H6 (l) = 49.0 kJ
ΔHof CO2 (g) = - 393.5 kJ
ΔHof H2O (l) = -285.8 k J
Which one of the following is not a state function ? change in temperature internal energy enthalpy heat Calculate ΔH for the following reaction C2H4 (g) + 6 F2 → 2 CF4 (g) + 4 HF (g) from H2 (g ) + F2 (g) → 2 HF (g) ΔH = - 537 kJ C (s) + 2 F2 (g) → CF4 (g) ΔH = -680 kJ 2 C (g) + 2 H2 (g) → C2H4 (g) ΔH = + 52 kJ...
The balanced combustion reaction for C6H6 is 2 C6H6(l) + 15 O2 (g) -----> 12 CO2 (g) + 6 H2O(l) + 6542 kJ If 8.800 g C6H6 is burned and the heat produced from the burning is added to 5691 g of water at 21 C, What is the final temperature of the water? final temperature= ___________ C
2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) Compound ΔHof (kJ/mol) Sof (J/mol.K) H2S(g) -20.6 205.8 O2(g) 0 205.2 H2O(l) -285.8 70.0 SO2(g) -296.8 248.2 1.Calculate ΔHrxn. 2.Calculate ΔSsurroundings. 3Calculate ΔSuniverse.
Consider the following reaction: C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(g) ΔHo = -1428 kJ The enthalpy of vaporization (ΔHovap) of water is 41 kJ/mol. What will ΔHo be for the reaction above if liquid water is formed instead of water vapor?
Standard Enthalpies of Formation (ΔHof): C4H10(g) = -124.8 kJ/mol CO2(g) = -393.5 kJ/mol H2O(l) = -285.8 kJ/mol What is the total amount of heat required for the process? What is the molar heat of combustion for butane? What is the mass of butane needed for this process?
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
loab beboo 2CO2 + H2O. 7. Calculate AH for C2H2 +5/202 Given C(s) +O2(g) CO2(g) AH = -393.5 kJ H2+½ O2 H2O AH= -285.8 kJ 2C+H2 C2H2 AH = 226.8 kJ 008700000 08.0 Lon Qoe cOeEo.O60
From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn = –726.4 kJ/mol C(graphite) + O2(g) → CO2(g) ΔHorxn = –393.5 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔHorxn = –285.8 kJ/mol Calculate the enthalpy of formation of methanol (CH3OH) from its elements. C(graphite) + 2H2(g) + ½O2(g) → CH3OH(l) Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines. From...
Use Hess’s law to calculate ∆H° for the reaction:C(s) + 2H2(g) + ½O2(g) → CH3OH(l) ∆H°∘= ?using only the following data:H2(g) + ½O2(g) → H2O(l) ∆H°= -285.8 kJC(s) + O2(g) → CO2(g) ∆H°= -393.5 kJ2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(l) ∆H°= -1452.8 kJ
9.Enter your answer in the provided box. S(rhombic) + O2(g) → SO2(g) ΔHo rxn= −296.06 kJ/mol S(monoclinic) + O2(g) → SO2(g) ΔHo rxn= −296.36 kJ/mol calculate the enthalpy change for the transformation S(rhombic) → S(monoclinic) (Monoclinic and rhombic are different allotropic forms of elemental sulfur.) _______kJ/mol 10. Enter your answer in the provided box Use the following data to calculate ΔHo/f for CS2(l): C(graphite) + O2(g) → CO2(g) ΔHo rxn= −393.5 kJ/mol S(rhombic) + O2(g) → SO2(g) ΔHo rxn=...