For the reaction whose reactants and products are:
reactants: NO (g) H2O (g)
products: NH3 (g) O2 (g)
calculate the standard free energy change (kJ/mole) from the standard free energies of formation.
i got 1319.432 and it was wrong. can someone show me what i did wrong.
2007-03-01 05:16:34 · 4 answers · asked by xdmandyxp 1 in Science & Mathematics ➔ Chemistry
the equation i got was 4NO + 6H2O -> 4NH3 + 5O2.
( (4 x 16.45) + 5(0) ) - (4 x 86.55) - (6 x - 288.572)
it got the answer i stated before and it was wrong.
2007-03-01 05:30:38 · update #1
Did you use the correct balanced equation, I wonder? And multiply the enthalpies of formation by the correct number of moles?
4NH3 + 5O2 ----> 4NO + 6H2O
Is the normal equation. You seem to want it backwards, too.
2007-03-01 05:27:19 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
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2016-05-16 03:42:11 · answer #2 · answered by ? 4 · 0⤊ 0⤋
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2016-10-17 00:46:10 · answer #3 · answered by ? 4 · 0⤊ 0⤋
there's nothing wrong with the balance you have a mistake with the h2o DG ...and try to keep everything in their right signs so you don't get confuse....the answer is a positive #....hope this helps
2007-03-01 15:25:14 · answer #4 · answered by kenneth x 3 · 0⤊ 0⤋