Hess' cycle for C2H4(g) + HBr(g) → C2H5Br(g)Watch
HBr(g) –36.2 ΔHf/kJ mol–1
C2H5Br(g)–60.4 ΔHf/kJ mol–1
Use the data in the table above to calculate the standard enthalpy change for the following reaction.
C2H4(g) + HBr(g) → C2H5Br(g)
I already have the answer for this but I am very stuck on what the products would be at bottom of hess' cycle because there is a bromine attached to the hydrogen and not just hydrogen gas which forms straight H2O, can anyone help me please?
1/2C! This is what I generally do.
It's a controversial concept in chemistry, also it probably doesn't matter if it's not balanced.