Of course I don't know the contents of Table 6.2.
For 2 mols NH3 the equation is
N2 + 3H2 ==> 2NH3 (for 2 mols) dH = -46.11*2 kJ
1/2 N2 + 3/2 H2 ==> NH3 (for 1 mol) dH = -46.11 kJ
You should add (g) to each to show the phase.
I don't know how you got 0. My tables show dHof for NH3 = -46.11 kJ/mol and of course zero for H2 and N2.
I don't know what summation equations are looking at.
1N2(g) reacts with H2(g) to form NH3(g), gaseous ammonia.
Show balanced thermochemical equations based on both one mole and two moles of NH3(g).
Determine Ho ( for both reactions using Table 6.2 (Hof).
Use the summation equations.
Show your calculations
N2 +H2 NH3 when I looked up the standard enthalpies of formation at 25 degrees the numbers came out to be 0. I don't know how to even set this up. Do I balance the equation?
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