Propane (C3H8) is burned in oxygen to pro-

duce carbon dioxide and water. The heat of
combustion of propane is -2012 kJ/mole. How
much heat is given off when 3.0 mol C3H8 are
reacted with 10.0 mol O2?
1. 4024 kJ
2. 2012 kJ
3. 916 kJ
4. 1555 kJ
5. 5122 kJ
6. 672 kJ
7. 6036 kJ
8. 7392 kJ

Another limiting reagent problem. Determine which is the limiting reagent. Use to determine how much C3H8 was used.

2012 kJ/mol x mol C3H8 used = ? kJ.

Well, it seems like propane is getting all fired up in this question! So, let's calculate the heat produced when 3.0 moles of C3H8 are reacted with 10.0 moles of O2.

First, we need to determine the limiting reactant. Since O2 is present in excess, we can look at the balanced chemical equation to determine the moles of O2 needed to react with 3.0 moles of C3H8.

From the balanced equation:

C3H8 + 5O2 -> 3CO2 + 4H2O

We see that it takes 5 moles of O2 to react with 1 mole of C3H8. So, for 3.0 moles of C3H8, we would need 3.0 * 5 = 15.0 moles of O2.

Since we have only 10.0 moles of O2, we can see that O2 is the limiting reactant.

Now let's calculate the heat of combustion using the given heat of combustion for propane (-2012 kJ/mol).

Since 3 moles of C3H8 are burned, we multiply the heat of combustion by 3:

-2012 kJ/mol * 3 mol = -6036 kJ

And there you have it! The amount of heat given off when 3.0 moles of C3H8 are reacted with 10.0 moles of O2 is -6036 kJ. So, option 7 (6036 kJ) is the correct answer.

Now, isn't that a hot result? The heat is really cooking!

To find out how much heat is given off when 3.0 mol of C3H8 are reacted with 10.0 mol of O2, we need to calculate the moles of CO2 and H2O produced, and then use the heat of combustion of propane.

The balanced equation for the combustion of propane is:
C3H8 + 5O2 -> 3CO2 + 4H2O

From the balanced equation, we can see that for every 1 mol of C3H8 burned, 3 mols of CO2 are produced.

Therefore, when 3.0 mol of C3H8 are burned, the moles of CO2 produced can be calculated as:
3.0 mol C3H8 * 3 mol CO2 / 1 mol C3H8 = 9.0 mol CO2

Since the heat of combustion of propane is given as -2012 kJ/mol, the heat released for 3.0 mol of C3H8 can be calculated as:
9.0 mol CO2 * (-2012 kJ/mol) = -18108 kJ

So, when 3.0 mol of C3H8 are reacted with 10.0 mol of O2, the heat given off is -18108 kJ.

However, since heat is usually expressed as a positive value, we can write the answer in positive form as 18108 kJ.

Therefore, the correct answer is not provided in the answer choices.

To solve this problem, you need to use the stoichiometry of the reaction and the heat of combustion of propane.

The balanced equation for the combustion of propane is:

C3H8 + 5O2 -> 3CO2 + 4H2O

From the balanced equation, you can see that 1 mole of propane reacts with 5 moles of oxygen to produce 3 moles of carbon dioxide and 4 moles of water.

Given that the heat of combustion of propane is -2012 kJ/mole, it means that for every mole of propane burned, 2012 kJ of heat is released.

To find out how much heat is given off when 3 moles of propane are reacted with 10 moles of oxygen, you need to calculate the moles of propane burned and then multiply it by the heat of combustion.

Since the balanced equation tells you that 1 mole of propane reacts with 5 moles of oxygen, you can calculate the moles of propane burned by dividing the moles of oxygen by 5.

10 moles of oxygen / 5 = 2 moles of propane

Now that you know you have 2 moles of propane, you can multiply it by the heat of combustion of propane.

2 moles of propane * -2012 kJ/mole = -4024 kJ

Since the heat of combustion is a negative value (indicating that it is released), the answer is 4024 kJ.

Therefore, the correct answer is 1. 4024 kJ.