Question

When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00 atm, H2O (l)...

When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00 atm, H2O (l) and CO2 (g) are formed with the evolution of 50.33 kJ of energy.

Substance

∆Hºf (kJ mol -1)

Sº (J mol -1 K -1)

H2O (l)

- 285.8

69.95

CO2 (g)

- 393.5

213.7

O2 (g)

0.0

205.0

C3H8 (g)

?

270.2

Calculate the molar enthalpy of combustion, ∆Hºcomb , of propane and the standard molar enthalpy of formation, ∆Hºf , of propane gas.
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The combustion reaction of propane is given by:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l)

No. of moles of Propane = Mass/Molar Mass

                                    = 1/44 = 0.023 mole

Molar Enthalpy of Combustion of propane,

Standard Molar Enthalpy of Formation of propane =

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8)...
At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8) was burned, producing 15.7 g of CO2. What was the mole fraction of each gas in the mixture? Assume complete combustion.
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l) (unbalanced) ΔHf C2H6 (g) = -84.7 kJ/mol; S C2H6 (g) = 229.5 J/K⋅mol; ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S CO2 (g) = 213.6 J/K⋅mol; ΔHf H2O (l) = -285.8 kJ/mol; SH2O (l) = 69.9 J/K⋅mol; SO2 (g) = 205.0 J/K⋅mol
A sample of solid azulene (C10H8) that weighs 0.4925 g is burned in an excess of...
A sample of solid azulene (C10H8) that weighs 0.4925 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.150 °C. The heat capacity of the calorimeter and its contents is known to be 9.455×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or...
13. Propane burns in air according to the following equation: C3H8 (g) + 5 O2 (g)...
13. Propane burns in air according to the following equation: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) ∆H = -2043 kJ If 5.00 g of propane are reacted at a constant pressure of 1.15 atm leading to a change in volume of +8.6 L, calculate ∆E and the work done (in kJ). (MM C3H8 = 44.09 g/mol). Using the information given (∆Hrxn = -2043 kJ) and any needed values from you text, calculate...
The standard enthalpy change for the combustion of 1 mole of ethylene is -1303.1 kJ C2H4(g)...
The standard enthalpy change for the combustion of 1 mole of ethylene is -1303.1 kJ C2H4(g) + 3 O2(g) ----> 2 CO2(g) + 2 H2O Calculate the change of Hf for ethylene based on the following standard molar enthalpies of formation. molecules Change in Hf (kJ/mol) CO2 -393.5 H2O -241.8
3. Use the enthalpies of formation in the table below to answer the following questions. Substance...
3. Use the enthalpies of formation in the table below to answer the following questions. Substance Enthalpy of Formation (kJ/mol), 298 K Oxygen (O2)(g) 0 Methane (CH4)(g) -74.8 Carbon Dioxide (CO2)(g) -393.5 Water (H2O)(g) -241.8 Water (H2O)(l) -285.8 a) Calculate the change in enthalpy for the combustion of methane using the values in the table above (assuming that the system remains at 298 K) for the combustion of methane to form carbon dioxide and gaseous water. b) Repeat this calculation...
A sample of asparagine was burned in the bomb calorimeter calibrated above. The following energy value...
A sample of asparagine was burned in the bomb calorimeter calibrated above. The following energy value was determined for the balanced reaction: 2 C4H8N2O3(s) + 13 O2(g) → 8 CO2(g) + 8 H2O(l) + 4 NO2(g) ΔrU = -3720 kJ Calculate the enthalpy of formation for solid asparagine, ΔfH(C4H8N2O3, ΔfH(CO2, g) = -393.52 kJ/mol ΔfH(H2O, l) = -285.83 kJ/mo lΔfH(NO2, g) = +33.10 kJ/mol Assume that ΔrU= ΔrH The answer is -790 kJ/mol enthalpy of formation solid asparagine 1. What...
Calculate the deltaH rxn for the production of CO2 and H20 via propane combustion, using thermochemical...
Calculate the deltaH rxn for the production of CO2 and H20 via propane combustion, using thermochemical equations below. Show all work! 3 C (s) + 4 H2 (g) = C3H8 (g) Delta H = (-) 103.9 kJ/mol C (s) + O2 (g) = CO2 (g) Delta H = (-) 393.5 kJ/mol H2 (g) + 1/2 O2 (g) = H2O (g) Delta H = (-)241. 8 kJ/mol Delta H rxn : ?
Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from...
Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from Appendix C, calculate the standard enthalpy of formation of acetone. Complete combustion of 1 mol of acetone (C3H6O) liberates 1790 kJ: C3H6O(l)+4O2(g)?3CO2(g)+3H2O(l)?H?=?1790kJ
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 heat of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT