SF4 we break 4 SF bonds. That times 2.
O2 we break 1 O2 bond. That times 1.
OSF4. We form 4 S-F bonds and 1 S=O bond. That times 2.
Then BE reactants - BE products = delta H rxn.
Plz explain in detail....
i tried to search on internet but i am confused with co-efficents.. how to set up the equaiton .. plz help me ???
Bond enthalpy is the energy required to break a mole of a certain type of bond.
O=O = 495 kj/mol
S-F = 327 kj/mol
S=O = 523 kj/mol
Use average bond enthalpies to estimate the enthalpy delta H (rxn) of the following reaction:
2SF4 + O2 ---- 2OSF4
Express your answer numerically in kilojoules.
Thanks in Advance
3 answers
can u plz figure out the answer for me .. its very urgent.. thnks ..
i still didn't get it
thnks a lot Dr bob
i still didn't get it
thnks a lot Dr bob
Just plug in the numbers and punch your calculator. The idea here is to show you how to do it, not to do it for you.
1 answer