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

How much energy (in kJ) is released if 15.6 g of ethaneundergoes combustion?

(Give your answer as a positive number.)

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Related questions

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

Part A If 1.00 mol of ethane gas and 2.40 mol of oxygen gas react, what is the limiting reactant? 2C2H6(g)+7O2(g)→4CO2(g)+6H2O(g) If 1.00 of ethane gas and 2.40 of oxygen gas react, what is the limiting reactant?

a.) O2

b.) C2H6

c.) neither C2H6 nor O2

Part B

How many moles of water are produced according?

1.A hydrated form of copper sulfate (CuSO4·x H2O) is heated to drive off all the water. If we start with 9.19 g of hydrated salt and have 5.87 g of anhydrous CuSO4 after heating, find the number of water molecules associated with each CuSO4 formula unit.

2.Iron(II) Sulfate forms a blue-green hydrate with the formula FeSO4 ·n H2O(s). If this hydrate is heated to a high enough temperature, H2O(g) can be driven off, leaving the dirty yellow anhydrous salt FeSO4(s). A 18.300-g sample of the hydrate was heated to 300 °C. The resulting FeSO4(s) had a mass of 9.9993 g. Calculate the value of n in FeSO4 ·n H2O(s).

3.The combustion of ethane (C2H6) produces carbon dioxide and steam:

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

How many moles of CO2 are produced when 5.15 mol of ethane are burned in an excess of oxygen?

--------MOLS?

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