CH4 + O2 = CO2 + H2O AND the change in heat is minus 890. Now the question is what is the energy bond of (C=O)?
To determine the energy bond of the carbon-oxygen (C=O) bond in carbon dioxide (CO2), we need to calculate the bond energy. Bond energy is the amount of energy required to break a particular bond.
To find the bond energy of the C=O bond, we can use the given information about the change in heat (∆H) during the combustion reaction of CH4 to CO2 and H2O. In this reaction, we know that ∆H is -890 kJ/mol.
First, let's consider the combustion reaction equation: CH4 + O2 → CO2 + H2O
From the balanced equation, we see that one molecule of CH4 produces one molecule of CO2. This means that the -890 kJ of energy released is for one mole of CO2 formed.
Now, we know that the combustion of CH4 forms one mole of CO2, which means that the -890 kJ of energy release is for one mole of CH4 combusted.
Therefore, we can conclude that the energy released during the combustion of one mole of CH4 is the same energy required to break the C=O bond in one mole of CO2.
Hence, the bond energy of the C=O bond in carbon dioxide (CO2) is -890 kJ/mol.
Note: The negative sign indicates that energy is released during the formation of the bond.