Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:
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 kcal
b) C2H6(g) + (7/2)O2(g) → 2CO2(g) + 3H2O(l), ΔH = -373 kcal
c) H2(g) + (1/2)O2(g) → H2O(l), ΔH = -68.3 kcal
Homework Answers
According to the Hess' Law of constant heat summation, if we wish to calculate the heat of formation of a product which is formed in multiple steps then the required change in the enthalpy will be the sum of the change in enthalpies of every individual step.
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Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:
problem is together. 3. Calculate the enthalpy of formation of carbon dioxide in the following reaction:...
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
Part 1) Use the following equations to calculate the heat of the reaction for the formation...
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 find the standard enthalpy change for the reaction CO2(g) → C(s) +...
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
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the...
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the reaction: 6 C (s) + 7 H2(g) → C6H14 (l) ΔHrxn = ? C6H14 (l)+19/2O2 (g)→6CO2(g)+ 7H2O(g). ΔH=–3505.8kJ C(s) + O2 (g) → CO2(g) ΔH=–393.5kJ H2(g) + 1/2 O2(g) → H2O(g). ΔH = – 242.0 kJ
Find the change in enthalpy for the reaction below, given the following reactions and change in...
Find the change in enthalpy for the reaction below, given the following reactions and change in enthalpy values: C2H2(g)+ 5/202(g)-2CO2(g) + H2O(g) ΔΗ ? Use: C2H6(g) → C2H2(g) + 2H2(g) ΔΗ : 283.5 kJ H29) 1/2029) H20(g) AH--213.7 kJ 2CO2(g) + 3H2O(g)-C2H6(g) + 7/2O2(g) ΔΗ = 849 kJ
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) +...
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
Find the mass of ethane C2H6 required to produce 5000 kJ of heat. C2H6(g) + 7...
Find the mass of ethane C2H6 required to produce 5000 kJ of heat. C2H6(g) + 7 2O2(g) = 2CO2(g) + 3H2O(g), ∆H◦ = −1423 kJ/mol. (C2H6) = 30.07 g/mol.
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
Imported From Sa... 4. Use Hess' Law to calculate the enthalpy change (AHY) for this reaction:...
Imported From Sa... 4. Use Hess' Law to calculate the enthalpy change (AHY) for this reaction: (12 pts.) 6C) + 6H21 309) CH120) using the following equations: A. Cw+ O2(g) → CO2(0) B. Hag) + 1/2O2(g) → H2O(g) C. CoH12O6 + 602(0)+ 6CO2(g) + 6H2O D. H2O → H2O(g) AH'= -393.5 kJ SH-241.8kJ AH = -2803.0 kJ AH = +40.71 kJ Why is this change in enthalpy given the term AHY? (3 pts.)
Use the following information and hess's law to find the enthalpy change for the reaction C(g)...
Use the following information and hess's law to find the enthalpy change for the reaction C(g) + O2(g) => CO2(g) reaction 1: 2CO(g) + O2(g) => 2CO2(g) ΔH = -566 kj reaction 2: 2C(g) + O2(g) => 2CO(g) ΔH = -1655 kj
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
Find the change in enthalpy for the reaction below, given the following reactions and change in enthalpy values: C2H2(g)+ 5/202(g)-2CO2(g) + H2O(g) ΔΗ ? Use: C2H6(g) → C2H2(g) + 2H2(g) ΔΗ : 283.5 kJ H29) 1/2029) H20(g) AH--213.7 kJ 2CO2(g) + 3H2O(g)-C2H6(g) + 7/2O2(g) ΔΗ = 849 kJ
Imported From Sa... 4. Use Hess' Law to calculate the enthalpy change (AHY) for this reaction: (12 pts.) 6C) + 6H21 309) CH120) using the following equations: A. Cw+ O2(g) → CO2(0) B. Hag) + 1/2O2(g) → H2O(g) C. CoH12O6 + 602(0)+ 6CO2(g) + 6H2O D. H2O → H2O(g) AH'= -393.5 kJ SH-241.8kJ AH = -2803.0 kJ AH = +40.71 kJ Why is this change in enthalpy given the term AHY? (3 pts.)
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