How do you calculate the energy released when 1 mole of ethanol, C2H5OH, is burned?
Well, calculating the energy released when ethanol is burned is a piece of cake! Just make sure to wear oven mitts while doing it, because things might get a little heated.
First, we need to know the combustion equation for ethanol, which is:
C2H5OH + 3O2 → 2CO2 + 3H2O
Now, we need to find the enthalpy change of combustion (ΔHc) for ethanol. The value for ΔHc of ethanol is approximately -1367 kJ/mol.
Since one mole of ethanol is burned, we can say that the energy released will be around -1367 kJ.
But hey, keep in mind that this is just an estimate. So don't go using this as an excuse to start a bonfire with a bunch of ethanol. Safety first!
To calculate the energy released when 1 mole of ethanol, C2H5OH, is burned, you can use the concept of enthalpy of combustion.
Step 1: Write the balanced chemical equation for the combustion of ethanol:
C2H5OH + 3O2 -> 2CO2 + 3H2O
Step 2: Determine the standard enthalpy of combustion (∆H°comb) for ethanol. This is typically given in kJ/mol and represents the energy released when 1 mole of a substance is completely burned under standard conditions. The standard enthalpy of combustion for ethanol is approximately -1367 kJ/mol.
Step 3: Calculate the energy released when 1 mole of ethanol is burned by multiplying the ∆H°comb value by the stoichiometric coefficient of ethanol in the balanced equation. In this case, the stoichiometric coefficient of ethanol is 1.
-1367 kJ/mol * 1 mol of ethanol = -1367 kJ
Therefore, the energy released when 1 mole of ethanol is burned is approximately -1367 kJ. Note that the negative sign indicates that the reaction is exothermic, meaning energy is released.
To calculate the energy released when 1 mole of ethanol (C2H5OH) is burned, you can use the concept of enthalpy change of combustion. The enthalpy change of combustion (∆Hc) represents the energy released when a substance undergoes complete combustion.
Here's how you can calculate it:
Step 1: Write the balanced combustion equation.
The balanced equation for the combustion of ethanol is:
C2H5OH + 3O2 → 2CO2 + 3H2O
Step 2: Determine the molar mass of ethanol.
The molar mass of ethanol (C2H5OH) can be calculated by summing the atomic masses of carbon (C), hydrogen (H), and oxygen (O) in the molecule:
C: 12.01 g/mol
H: 1.01 g/mol (there are 6 hydrogens in ethanol)
O: 16.00 g/mol
Total molar mass of ethanol (C2H5OH): 2(12.01 g/mol) + 6(1.01 g/mol) + 16.00 g/mol = 46.07 g/mol
Step 3: Determine the heat of combustion per mole of ethanol (∆Hc per mole).
The heat of combustion, also known as the molar heat of combustion, represents the energy released per mole of the substance when undergoing combustion. The heat of combustion for ethanol is approximately -1367 kJ/mol.
Step 4: Calculate the energy released.
Using the equation:
Energy released = ∆Hc per mole × number of moles
Since we are considering 1 mole of ethanol, the energy released can be calculated as:
Energy released = -1367 kJ/mol × 1 mol = -1367 kJ
So, when 1 mole of ethanol is burned, approximately 1367 kJ of energy is released.
Note: The negative sign indicates the release of energy during combustion.