How much heat is absorbed/released when 35.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(l) according to the following chemical equation?
4NH3(g)+5O2(g)--->4NO(g)+6H2O(l)
DeltaH=1168kj
6 answers
i got 601.1 are released is that right?
Is that 1168 kJ/mole or 1168 kJ/reaction?
And is the problem not telling whether it is absorbed/released on purpose?
And is the problem not telling whether it is absorbed/released on purpose?
yeah it just says rleased/absorbed i guess that's what they want you to find out im not sure what you mean by 1168 kJ/mole or 1168 kJ/reaction?
Is that 1168 kJ for the reaction (4 moles NH3 or 68 grams) or kJ/mol (for 17 grams).
Yes, 601 kJ is right and it is released; i.e., the 1168 is -1168 kJ for the reaction as written.
1168 x (35.0/68) = 601 kJ released or delta H = -601 kJ.
1168 x (35.0/68) = 601 kJ released or delta H = -601 kJ.
428.6kJ of heat
2 answers