How much energy is released by the combustion of 1.00 mol of octane, C8H18?
Well, let's do the math, but let's keep it fun, shall we?
Okay, so octane combustion is like a party for atoms, but a very fiery one. Octane has 8 carbon atoms and 18 hydrogen atoms, and they all love to dance with oxygen to form carbon dioxide (CO2) and water (H2O).
Now, each carbon atom releases about 400 kJ/mol when it turns into carbon dioxide, and each hydrogen atom gives us about 286 kJ/mol when it turns into water. So, for every mole of octane, we would have 8 moles of carbon dioxide and 9 moles of water.
Calculating the energy, we'll find that the carbon dioxide gives us 3200 kJ/mol (8 x 400 kJ/mol), and the water gives us 2574 kJ/mol (18 x 286 kJ/mol). Adding these two values together, we get a whopping total of 5774 kJ/mol.
So, when 1.00 mol of octane (C8H18) is combusted, it releases approximately 5774 kJ of energy. That's enough to power a small circus, or maybe just your chemistry homework. Keep it fiery!
To determine the amount of energy released by the combustion of 1.00 mol of octane (C8H18), we can use the standard enthalpy of combustion (∆H°comb) for octane.
The balanced chemical equation for the combustion of octane is:
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
The standard enthalpy change (∆H°comb) for this reaction is -5471 kJ/mol of octane.
To calculate the energy released by the combustion of 1.00 mol of octane, we multiply the molar quantity by the ∆H°comb value:
Energy released = 1.00 mol of octane × -5471 kJ/mol of octane
This gives us the answer:
Energy released = -5471 kJ
Therefore, the combustion of 1.00 mol of octane releases 5471 kJ of energy.
To determine the energy released by the combustion of 1.00 mol of octane (C8H18), you need to use the balanced chemical equation for the combustion of octane and the corresponding enthalpy of combustion (ΔHcomb) value.
Here is the balanced chemical equation for the combustion of octane:
2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O
From this balanced equation, you can see that for every 2 moles of octane combusted, you get 16 moles of carbon dioxide and 18 moles of water.
Now, you need to find the enthalpy of combustion value for octane, which represents the amount of energy released when one mole of octane is completely burned. The enthalpy of combustion value for octane is -5471 kJ/mol.
To calculate the energy released by the combustion of 1.00 mol of octane, you can use the ratio:
ΔHcomb / 2 moles of octane = x kJ / 1 mole of octane
Plugging in the values:
-5471 kJ/mol / 2 mol of octane = x kJ / 1 mol of octane
Solving for x, you get:
x = (-5471 kJ/mol / 2 mol of octane) * 1 mol of octane
x = -2735.5 kJ
Therefore, the combustion of 1.00 mol of octane releases approximately 2,735.5 kJ of energy.
You can calculate this by
1. Write the equation and balance it.
2. Look up the delta Hf values in your text or notes for products and reactants
3. Then deltaHrxn = (n*DHproducts)-(n*DHreactants).
Post your work if you get stuck.