Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Rutherford on June 03, 2012, 10:06:28 AM
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Found on the IChO, and it seemed very interesting to me:
Calculate the Si–Si bond dissociation enthalpy of Si2H6 from the following informations:
Bond dissociation enthalpy for H–H = 436 kJ/mol
Bond dissociation enthalpy for Si–H = 304 kJ/mol
ΔfH [Si(g)] = 450 kJ/mol
ΔfH [Si2H6(g)] = 80.3 kJ/mol
2Si(g)+3H-H(g) :rarrow: H3Si-SiH3(g)
I have two expresions to calculate ΔH:
ΔH=ΔfH [Si2H6(g)] - 2ΔfH [Si(g)]
ΔH=3Bond dissociation enthalpy(H-H) - 6Bond dissociation enthalpy(Si-H) - Bond dissociation enthalpy(Si-Si)
And I got that the bond dissociation enthalpy(Si-Si)=303.7kJ/mol, but I found somewhere on the net that Si-Si=around 50. Did I calculate this wrong or not?
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50 is most probably in kcal/mol units.
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Is my calculation right?
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Robin Walsh
Acc. Chem. Res. 1981,14, 246-252
(Table 4) 74 kcal/mol= 309 kJ/mol
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I worked it out got the same result. I think we're right. Calculation seems legit to me
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Ok, thanks.