Question

1.) Describe the relationship between∆Esys and ∆Esurr,. 2.) Calculate ΔH° for the following reaction using standard...

1.) Describe the relationship between∆Esys and ∆Esurr,.

2.) Calculate ΔH° for the following reaction using standard enthalpies of formation.

2C2H6(g) + 7O2(g)—> 6H2O(g) + 4CO2(g)

Homework Answers

Answer #1

1)

Since Energy is conserved,

∆Etotal = 0

use:

∆Etotal = ∆Esys + ∆Esurr

∆Esys + ∆Esurr = 0

∆Esys = - ∆Esurr

They have same magnitude but opposite sign

2)

we have:

Hof(C2H6(g)) = -84.68 KJ/mol

Hof(O2(g)) = 0.0 KJ/mol

Hof(H2O(g)) = -241.818 KJ/mol

Hof(CO2(g)) = -393.509 KJ/mol

we have the Balanced chemical equation as:

2 C2H6(g) + 7 O2(g) ---> 6 H2O(g) + 4 CO2(g)

deltaHo rxn = 6*Hof(H2O(g)) + 4*Hof(CO2(g)) - 2*Hof( C2H6(g)) - 7*Hof(O2(g))

deltaHo rxn = 6*(-241.818) + 4*(-393.509) - 2*(-84.68) - 7*(0.0)

deltaHo rxn = -2856 KJ/mol

Answer: -2856 KJ/mol

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l)...
Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l)
For the reaction 2C2H6(g) + 7O2(g) ----> 4CO2(g) + 6H2O(g) ΔH° = -2855.4 kJ and ΔS°...
For the reaction 2C2H6(g) + 7O2(g) ----> 4CO2(g) + 6H2O(g) ΔH° = -2855.4 kJ and ΔS° = 92.7 J/K The maximum amount of work that could be done when 2.39 moles of C2H6(g) react at 349 K, 1 atm is ____ kJ. Assume that ΔH° and ΔS° are independent of temperature.
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction...
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction is the conversion of methane to ethylene: 2CH4(g)⟶C2H4(g)+2H2(g) Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l ΔH∘=−3120.8kJ
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction...
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction is the conversion of methane to ethylene: 2CH4(g)⟶C2H4(g)+2H2(g) Part A Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l) ΔH∘=−3120.8kJ Express your answer to four significant figures and include the appropriate units.
Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: SO2(g)+12O2(g)→SO3(g) ΔH∘rxn =
Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: SO2(g)+12O2(g)→SO3(g) ΔH∘rxn =
Consider the following balanced reaction: 2C2H6(g) + 7O2(g) ->4CO2(g) + 6H2O(g) How many liters of carbon...
Consider the following balanced reaction: 2C2H6(g) + 7O2(g) ->4CO2(g) + 6H2O(g) How many liters of carbon dioxide at STP are produced when 60.0 liters of C2H6 (g) are combusted?
1.Using the enthalpies of formation given below, calculate ΔH°rxn in kJ, for the following reaction. Report...
1.Using the enthalpies of formation given below, calculate ΔH°rxn in kJ, for the following reaction. Report your answer to two decimal places in standard notation. H2S(g) + 2O2(g) → SO3(g) + H2O(l) H2S (g): -20.60 kJ/mol O2 (g): 0.00 kJ/mol SO3 (g): -395.77 kJ/mol H2O (l): -285.83 kJ/mol 2. Calculate the amount of heat absorbed/released (in kJ) when 22.54 grams of SO3 are produced via the above reaction. Report your answer to two decimal places, and use appropriate signs to...
For the reaction 2C2H6(g) + 7O2(g)4CO2(g) + 6H2O(g) H° = -2855.4 kJ and S° = 92.7...
For the reaction 2C2H6(g) + 7O2(g)4CO2(g) + 6H2O(g) H° = -2855.4 kJ and S° = 92.7 J/K The standard free energy change for the reaction of 2.19 moles of C2H6(g) at 282 K, 1 atm would be ___ kJ. This reaction is (reactant, product) ____ favored under standard conditions at 282 K. Assume that H° and S° are independent of temperature.
Calculate the standard enthalpy change (ΔH⁰rxn ) for the reaction of TiCl4(g) and H2O(g) to form...
Calculate the standard enthalpy change (ΔH⁰rxn ) for the reaction of TiCl4(g) and H2O(g) to form TiO2(s) and HCl(g) given the standard enthalpies of formation (ΔH⁰f ) shown in the table below. (Include the sign of the value in your answer.)   kJ Compound ΔH⁰f  (kJ/mol) TiCl4(g) −763.2 H2O(g) −241.8 TiO2(s) −944.0 HCl(g) −92.3
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The...
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The enthalpy of formation of Fe3O4 is −1117 kJ/mol. 8 Al(s) + 3 Fe3O4(s) → 4 Al2O3(s) + 9 Fe(s) 2. a) Nitroglycerin is a powerful explosive, giving four different gases when detonated. 2 C3H5(NO3)3(l) → 3 N2(g) + 1/2 O2 (g) + 6 CO2(g) + 5 H2O(g) Given that the enthalpy of formation of nitroglycerin, ΔHf°, is −364 kJ/mol, calculate the energy (heat at...