I'm supposed to estimate the ΔH for

O
||
H2C=CH2 +O3(g)--- CH3CH(g) + O2(g)

and i got [4(432)+(614)+(1072)]-[3(413)+(347)+(745)+(358)+(467)] the answer i got was 182 but the answer was wrong and i'm not sure what i did wrong.

To estimate the enthalpy change (ΔH) for a reaction, you need to know the enthalpies of formation for each individual compound involved in the reaction. The enthalpy of formation represents the enthalpy change when one mole of a compound is formed from its elements in their standard state at a given temperature and pressure.

First, let's find the enthalpy change for each compound in the reaction:

1. O2(g): Look up the enthalpy of formation for O2(g) from a reliable source. Let's assume it is ΔHf = 0 kJ/mol.

2. H2C=CH2: Likewise, look up the enthalpy of formation for H2C=CH2 (ethylene). Let's assume it is ΔHf = +52 kJ/mol.

3. O3(g): Find the enthalpy of formation for O3(g). Let's assume it is ΔHf = +142 kJ/mol.

4. CH3CH(g): Find the enthalpy of formation for CH3CH(g) (propene). Let's assume it is ΔHf = +20 kJ/mol.

Now, substitute the values into the reaction:

ΔH = [ΔHf(CH3CH) + ΔHf(O2)] - [ΔHf(H2C=CH2) + ΔHf(O3)]

ΔH = [(+20 kJ/mol) + (0 kJ/mol)] - [(+52 kJ/mol) + (+142 kJ/mol)]

ΔH = [+20 kJ/mol + 0 kJ/mol] - [+52 kJ/mol + 142 kJ/mol]

ΔH = (+20 kJ/mol + 0 kJ/mol) - (+194 kJ/mol)

ΔH = +20 kJ/mol - 194 kJ/mol

ΔH = -174 kJ/mol

Therefore, the estimated enthalpy change (ΔH) for the given reaction is -174 kJ/mol.

The equation isn't balanced. Did you use bond energies or dHo values.