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

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.

can u plz figure out the answer for me .. its very urgent.. thnks ..

i still didn't get it

thnks a lot Dr bob

To estimate the enthalpy change (ΔH) of a reaction using bond enthalpies, you need to consider the bonds that are broken and formed in the reaction. The general approach involves the following steps:

Step 1: Identify the bonds that are broken in the reactants. In this case, the reaction has two SF4 molecules, which means you have to break two S-F bonds.

Step 2: Determine the bond enthalpy for each bond that is broken. The given bond enthalpy for S-F is 327 kJ/mol.

Step 3: Multiply the number of bonds broken by their respective bond enthalpies. In this case, since two S-F bonds are broken, the total energy required would be 2 * 327 kJ/mol = 654 kJ.

Step 4: Identify the bonds that are formed in the products. The reaction produces 2 OSF4 molecules, which means you will form two S=O bonds.

Step 5: Determine the bond enthalpy for each bond that is formed. The given bond enthalpy for S=O is 523 kJ/mol.

Step 6: Multiply the number of bonds formed by their respective bond enthalpies. Since two S=O bonds are formed, the total energy released would be 2 * 523 kJ/mol = 1046 kJ.

Step 7: Calculate the ΔH of the reaction by subtracting the energy released from the energy required: ΔH = Energy required - Energy released = 654 kJ - 1046 kJ = -392 kJ.

Therefore, the estimated enthalpy change of the reaction 2SF4 + O2 -> 2OSF4 is -392 kJ.

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.