Use the following information to calculate the heat of formation
of propane C3H8.
3 C (S-Graphite) + 4 H2 (g) —› C3H8 (g)
1. C (S-Graphite) + O2 (g) —› CO2 (g) ΔH = - 393.5 kJ
2. H2 (g) + ½ O2 (g) —› H2O (l) ΔH = - 285.8 kJ
3. C3H4 (g) + 4 O2 (g) —› 3 CO2 (g) + 2 H2O (l) ΔH = - 1937 kJ
4. C3H6 (g) + 9/2 O2 (g) —› 3 CO2 (g) + 3 H2O (g) ΔH = - 2007 kJ
5. C3H8 (g) + 5 O2 (g) —› CO2 (g) + 4 H2O (l) ΔH = - 2219.1 kJ
1. C (S-Graphite) + O2 (g) —› CO2 (g) ΔH = - 393.5 kJ --------> 1
2. H2 (g) + ½ O2 (g) —› H2O (l) ΔH = - 285.8 kJ --------------> 2
3. C3H4 (g) + 4 O2 (g) —› 3 CO2 (g) + 2 H2O (l) ΔH = - 1937 kJ --------------> 3
4. C3H6 (g) + 9/2 O2 (g) —› 3 CO2 (g) + 3 H2O (g) ΔH = - 2007 kJ -------------> 4
5. C3H8 (g) + 5 O2 (g) —› CO2 (g) + 4 H2O (l) ΔH = - 2219.1 kJ -------------> 5
equation 1 multifly with 3 and equation 2 multifly with 4
3C (S-Graphite) + 3O2 (g) —› 3CO2 (g) ΔH = - 1180.5 kJ --------> 1
4 H2 (g) + 2 O2 (g) ---------------> 4H2O (l) ΔH = - 1143.2kJ --------------> 2
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3C( S-Graphite) + 4H2(g) + 5O2(g) ----------> 3CO2(g) + 4H2O(l) ΔH = -2323.69KJ
C3H8 (g) + 5 O2 (g) ----------------->3CO2 (g) + 4 H2O (l) ΔH = - 2219.1 kJ ---------> 5 subtract
(-) (-) (-) (-) (+)
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3 C (S-Graphite) + 4 H2 (g)-----------------------------> C3H8 (g) ΔH = -104.59KJ
Use the following information to calculate the heat of formation of propane C3H8. 3 C (S-Graphite)...
Question 3 Propane (C3H8) undergoes combustion according to the following thermochemical equation: C3H8(g) + 5 O2(g) -- 3 CO2(g) + 4H2O(g) Arxn = -2043.0 kJ Substance Heat of Formation (kJ/mol) CO2(g) -393.5 H2O(g) -241.8 O2(g) 0 C3H8(g) ? Calculate the standard enthalpy of formation of propane C3H8 a. -104.7 kJ/mol ob. +1407.7 kJ/mol C. -1407.7 kJ/mol O d. +104.7 kJ/mol o e. -4190.7 kJ/mol
The combustion of propane, C3H8, occurs via the reaction C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) C3H8 (g)= -104.7 CO2(g)= −393.5 H2O(g)= −241.8 Calculate the enthalpy for the combustion of 1 mole of propane.
PROBLEM-SOLVING CLASS ACTIVITY 11 Use Hess's Law to calculate the enthalpy of formation of CH2OH: C(graphite) + 2 H2(g) + 1026) → CH2OH(1) Given the following data: CH2OH() • 02(9) + CO2(g) + 2H2O(1) AH°: -726.4 kJ/mol C(graphite). O2(g) → CO2(9) AH' = -393.5 kJ/mol H2(g) + 40269) → H2O(1) AH = -285.8 kJ/mol
5. Using standard heats of formation, calculate AH for 4 FeO (s) + O2(g) → 2 Fe2O3 (s) AH1 of FeO (s) = -272.0 kJ/mol AHºf of Fe2O3 (s) = -825.5 kJ/mol 3. Given 3 C (s) + 4 H2(g) → C3H8 (9) AH = -103.85 kJ/mol C(s) + O2(g) + CO2(g) AH = -393.5 kJ/mol H2 (g) + 12 O2(g) → H2O (1) AH = -285.8 kJ/mol find AH for C3H8 (g) + 5 O2(g) → 3 CO2 (g)...
Combustion of 2.5000 g of propane (C3H8) releases 115.75 kJ of heat when it is burned to form CO2 (g) and H2O (l). The standard formation enthalpies of CO2 (g) and H2O (l) are -393.5 kJ/mol and -285.5 kJ/mol respectively. Calculate the Hrxn for the combustion of propane in kJ/mol Calculate ∆?? ? for propane
Given the following heat of formation values, calculate the heat of reaction for the following: C3H8(g) + O2(g) CO2(g) + H2O(1). AfH values in kJ/mol: C3H8(g): -103.8, O2(g): 0, CO2(g): -393.5, H2O(l): -285.8. 3.613 x 102 kJ/mol -2.220 103 kJ/mol 1.413* 102 kJ/mol -5.755 x 102 kJ/mol If a lighter contains 4.0 mL of liquid butane (density of butane = 0.8 g/cm3), how much heat can we get out of it, from the combustion of butane? 2 C4H 10(g) +...
Part 1) Use the following equations to calculate the heat of the reaction for the formation of ethane (C2H6). C2H6(g) + 7/2 O2(g) → 2CO2(g) + 3 H2O(l) ∆ Ho = -1560 kJ C(gr) + O2(g) → CO2(g) ∆ Ho = -394 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆ Ho = -286 kJ Calculate ∆Ho for the following reaction: 2 C(gr) + 3H2(g) → C2H6(g) ethane Use kJ for your answer. ΔHo = Part 2) Find the heat of...
Use Hess's law to determine A.Hº for the reaction C3H4(g) + 2 H2(g) -> C3H8(8), given that Hy(8) + O2(8) — H2O(1) A Hº = -285.8 kJ mol-1 C3H4(8) + 402(g) — 3 CO2(g) + 2 H2O(1) A Hº = -1937 kJ mol-1 C3H2(g) + 5O2(g) — 3CO2(g) + 4H2O(1) A Hº = -2219.1 kJ mol-1
Using the following equation for the combustion of propane, calculate the amount of propane consumed if the reaction gave off 333 kJ heat. C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4 H2O(g) ΔH = -2044 kJ
Use the following data to calculate the standard enthalpy of formation of heptane, C7H16 (l). C7H16 (l) + 11 O2 (g → 7 CO2 (g) + 8 H2O (l) ΔH° = -4817 kJ/mol ΔHf° of CO2 (g) = -393.5 kJ/mol ΔHf° of H2O (l) = -285.8 kJ/mol A)-218.2 kJ/mol B)-468.1 kJ/mol C)-223.9 kJ/mol D)-447.8 kJ/mol E)-111.5 kJ/mol