00:01
I don't have access to the standard enthalpyes of formation that you do, but i do have access to a table of standard anthopies of formation that should be very similar to the ones that you have.
00:13
To estimate the change in enthalpy for this reaction under standard states, what we do is we take the enthalpy of formation of the products multiplied by their coefficients minus the enthalpy of formation.
00:30
Of the reactants, but all of the coefficients here are one.
00:36
So delta h standard will be equal to the delta h of formation of carbon monoxide.
00:44
And in the table i have, the delta h of formation of carbon monoxide standard is negative 110 .5 kilojoules per mole, plus that for hydrogen, which is zero, minus that for carbon, assuming it's graphite, is zero.
01:09
Still minus, in the parentheses, the delta h of formation of gaseous water.
01:16
Remember to do gaseous water and not liquid water.
01:20
And the delta h, a formation in my table, is negative 242 kilojoules per mole.
01:28
And we get a delta h standard of 131 .5 kilojoules...