What is delta h for reaction between h2o2 and ethene to give ethylene glycol if HO-OH is 49 kcal/mol and C=C 65 kcal/mol
Please show ur work
To calculate the ΔH (enthalpy change) for the reaction between H2O2 and ethene to give ethylene glycol, we need to use the bond enthalpy values of the bonds broken and formed in the reaction.
The balanced equation for the reaction is:
H2O2 + C2H4 → HO-CH2-CH2-OH
Step 1: Calculate the ΔH for bonds broken (reactants)
In the reactants, two H-O bonds are broken in H2O2, and one C=C bond is broken in C2H4.
Bond enthalpy values:
H-O bond = 49 kcal/mol
C=C bond = 65 kcal/mol
ΔH for bonds broken = (2 * H-O bond) + (1 * C=C bond)
= (2 * 49 kcal/mol) + (1 * 65 kcal/mol)
= 98 kcal/mol + 65 kcal/mol
= 163 kcal/mol
Step 2: Calculate the ΔH for bonds formed (products)
In the product, we have one HO-CH2-OH bond formed.
Bond enthalpy value:
HO-CH2-OH bond = unknown
Step 3: Calculate the overall ΔH for the reaction
ΔH for the reaction = ΔH for bonds broken - ΔH for bonds formed
= 163 kcal/mol - (HO-CH2-OH bond)
Unfortunately, the bond enthalpy value for the HO-CH2-OH bond is not given in the question, so we are unable to calculate the overall ΔH for the reaction.