methane(g) +water= carbon monoxide(g)+Hydrogen (g)
use the bond energies in the following table to predict the delta H foe the reaction
No table included.
Take the sum of the B.E for bonds broken on the reactants side subtract the sum of the B. E, formed on the product side to calculate dHrxn
To predict the delta H for the given reaction, we need to consider the bond energies of the molecules involved. The bond energies can be found in a table that provides the average energy required to break a particular bond in a molecule.
Unfortunately, you mentioned a table without actually providing it. Without the specific bond energies table, I am unable to give you an accurate value for delta H. However, I can guide you on how to calculate it once you have the correct bond energies.
Here's the general approach to calculate delta H using bond energies:
1. Identify the bonds broken and formed in the reaction. In this case, methane (CH4) is breaking into carbon monoxide (CO) and hydrogen (H2) gas. Thus, the bonds broken are the C-H bonds in methane, and the bonds formed are the C-O bond in carbon monoxide and the H-H bond in hydrogen gas.
2. Look up the bond energies for each bond involved in the reaction. Bond energies are typically given in kilojoules per mole (kJ/mol). Make sure to use the correct values from your bond energies table.
3. Calculate the total energy required to break the bonds in the reactants and the total energy released when the bonds are formed in the products. Multiply the number of bonds by their respective bond energies.
4. Subtract the total energy released from the total energy required to obtain the value of delta H. The result will be in units of energy per mole (kJ/mol).
Remember to consider the stoichiometric coefficients of the reactants and products when calculating the bond energies.
If you provide the specific bond energies table you are referring to, I would be able to help you calculate the delta H for the reaction.