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 formation for a mole
of sulfuric acid given:
SO3(g) + H2O(l) → H2SO4(l) | ∆ Ho = -132.6 kJ | |
H2(g) + 1/2O2(g) → H2O(l) | ∆ Ho = -285.8 kJ | |
S(s) + 3/2O2(g)→SO3(g) | Δ Ho= -395.6 kJ |
Use kJ and 3 significant figures for your answer.
ΔHof of sulfuric acid =
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Part 1) Use the following equations to calculate the heat of the reaction for the formation...
Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:a) 2C(S) + 2O2(g) → 2CO2(g), ΔH = -188 kcalb) C2H6(g) + (7/2)O2(g) → 2CO2(g) + 3H2O(l), ΔH = -373 kcalc) H2(g) + (1/2)O2(g) → H2O(l), ΔH = -68.3 kcal
problem is together. 3. Calculate the enthalpy of formation of carbon dioxide in the following reaction: C(s) + O2(g) - CO, (g) Use the following equations: a) H2O(l) → H2(g) + 2O2(g) AH°-= +285.8 kJ/mol b) C2H6(g) → 2C (s) + 3H2(g) AH'= +84.7 kJ/mol c) 2CO2 (g) +3H2O (1) C2H6(g) + (7/2) O2(g) AH°F = +1560.7 kJ/mol
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) —›...
Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction: 2 C5H10O(g) + 19 O2(g) => 10 CO2(g) + 10 H2O(g) ΔHof C5H10O(g) = -232.11 kJ/mol Δ Hof CO2(g) = -393.5 kJ/mol ΔHof H2O(g) = -241.8 kJ/mol
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data. C2H4 (g) + 3 02 (®) → 2 CO2 (s) + 2 H20 (1) C2H6 (g) + 7/2 02(g) → 2 CO2(g) + 3 H20 (1) H2 + 1/2O2() → H20 (1) AH = -1411. kJ/mole AH = -1560. kJ/mole AH = -285.8 kJ/mole 2. Calculate AH for the reaction 4 NH3(g) +502 (g) → 4 NO(g) + 6 H20 (g), from the following...
1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1560 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1411 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 571.6 kJ/mol How much heat is transferred between the system and the surroundings when 25 grams of ethane (C2H6) decomposes to produce ethylene (C2H4) and...
1. From the following equations and enthalpies, determine the molar heat of formation of HNO2(aq) . NH4NO2(aq) → N2(g) + 2H2O(l) ∆H = -320.1 kJ NH3(aq) + HNO2(aq) → NH4NO2(aq) ∆H = -37.7 kJ 2NH3(aq) → N2(g) + 3H2(g) ∆H = +169.9 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆H = -285.8 kJ
Heat of Formation Calculations: 32) Use a standard enthalpies of formation (Ho) table to determine the change in enthalpy for each of these reactions Hrxn [n. Ho(products) - n. Ho(products)] CO (g): -110.5 kJ/mol; CO2 (g): -393.5 kJ/mol CH4 (g): -890.4 kJ/mol H2O (l): -285.8 kJ/mol; H2O (g): -241.8 kJ/mol H2S (g): -20.6 kJ/mol; NO: -90.2 kJ/mol NO2: +33.9 kJ/mol; HCl (g): -92.3 kJ/mol NaOH (s): -426.7 kJ/mol; SO2 (g): -296.8 kJ/mol a) CH4(g) + 2 O2(g) ---> CO2(g) +...
Use Hess’s Law to find the standard enthalpy change for the reaction CO2(g) → C(s) + O2(g) using only the following information. Show all your work, including any equations you use to obtain your answer and showing clearly how you obtained that answer. (3 pts.) H2O(l) → H2(g) + 1/2O2(g) C2H6(g) → 2C(s)+ 3H2(g) 2CO2(g) + 3H2O(l) → C 2H6(g) + 7/2O2(g) ∆Ho (kJ) 643 kJ 190.6kJ 3511.1 kJ
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...