Hydrogen cyanide is produced in the following balanced reaction.
2NH3 (g) + 3O2 (g) + 2CH4 (g) → 2HCN (g) + 6H2O (g)
Given the following standard heats of formation, calculate the approximate ΔH°rxn of this reaction.
Substance
ΔHf°(kJ/mol)
NH3
-46
CH4
-75
HCN
135
H2O
-242
Choose one answer.
a. -500 kJ
b. -1000 kJ
c. 500 kJ
d. -1500 kJ
e. -4519
f. not enough information is given to make the calculation
4 answers
dHrxn = (n*dHf products) - (n*dHf reactants)
When i did that I got -940 kJ but that isn't and option and neither is -1000kJ. So by default would the answer be F.
No, I wouldn't do that because there is enough information to actually calculate the delta H reaction. I ran through the calculation and came up with -940 kJ also so I would pick the closest answer which is -1000 kJ
Okay... but I tried that answer and it was incorrect.
1 answer