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13 Dec 2019

2C2H6 (g) + 7O2 (g) ?4CO2(g) + 6H2O (g) ?H = -1560 kJ

How much energy (in kJ) is released if 13.4 g of ethaneundergoes combustion?

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Sixta Kovacek
Sixta KovacekLv2
17 Dec 2019

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Related questions

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2.) 26.7 mol HCl in 90.0 L of solution. Express your answer with the appropriate units.

3.) 6.40×10−2 mol Li2CO3 in 696 mL of solution. Express your answer with the appropriate units.

4.) Ethane burns in air to form carbon dioxide and water. The equation is 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)

Part A In the above equation, how many liters of oxygen (O2) are required to burn 6.0 L of ethane (C2H6) gas? Assume that both gases are measured at the same temperature and pressure.Express your answer with the appropriate units.

Part B 2C2H6(g)+7O2(g)→4CO2(g)+6H2O(g) In the equation above, what volume of ethane (C2H6) in liters is required to form 24 L of carbon dioxide (CO2)? Express your answer with the appropriate units.

5.) 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g) In the equation, if 14 L of ethane (C2H6) and 14 L of oxygen (O2) combined and burned to completion, which gas will be leftover after the reaction, and what is the volume of that gas remaining? Enter the name of the gas followed by its volume in liters to the nearest whole number, separated by a comma.

A Comparison of Average Enthalpy (BE) and Heat of Formation:

Please answer both A and B of the following problem below:

For the reaction: 2C2H6(g) + 7O2(g) - 4CO2(g) + 6H2O(g)

A) Predict the enthalpy of reaction from the average bond energies

B) Calculate the enthalpy of reaction from the standard enthalpies of formation of the reactant and product molecules and compare the results with your answer for part A

Hint: for part (a) Ho = total energy input – total energy released

Hint for part (b) ) Ho = summation of products – summation of reactants

Heats of formation here: Ho C2H6(g) = -84.7 kJ/mol, Ho CO2 = -393.5 kJ/mol, Ho H2O = -241.8 kJ/mol

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