Values of measured bond energies may vary greatly depending on the molecule studied. Consider the following reactions: N C l 3 ( g ) → N C l 2 ( g ) + C l ( g ) Δ E = 375 k J / m o l O N C l ( g ) → N O ( g ) + C l ( g ) Δ E = 158 k J / m o l Rationalize the difference in the values of ∆ E for these reactions, even though each reaction appears to involve only the breaking of one N—Cl bond. (Hint: Consider the bond order of the NO bond in ONCl and in NO.)
Values of measured bond energies may vary greatly depending on the molecule studied. Consider the following reactions: N C l 3 ( g ) → N C l 2 ( g ) + C l ( g ) Δ E = 375 k J / m o l O N C l ( g ) → N O ( g ) + C l ( g ) Δ E = 158 k J / m o l Rationalize the difference in the values of ∆ E for these reactions, even though each reaction appears to involve only the breaking of one N—Cl bond. (Hint: Consider the bond order of the NO bond in ONCl and in NO.)
Solution Summary: The author explains the difference in the values of Delta E for the given reactions.
Values of measured bond energies may vary greatly depending on the molecule studied. Consider the following reactions:
N
C
l
3
(
g
)
→
N
C
l
2
(
g
)
+
C
l
(
g
)
Δ
E
=
375
k
J
/
m
o
l
O
N
C
l
(
g
)
→
N
O
(
g
)
+
C
l
(
g
)
Δ
E
=
158
k
J
/
m
o
l
Rationalize the difference in the values of ∆E for these reactions, even though each reaction appears to involve only the breaking of one N—Cl bond. (Hint: Consider the bond order of the NO bond in ONCl and in NO.)
Hydrazine, N2H4, burns in oxygen as follows:
N2H4 + O2 → N2 + 2H2O
[The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496]
Draw the chemical structures of the reactants and products and
give the formula to calculate enthalpy change in a reaction, ΔH.
Fructose, C6H1206(S), consists of 5 C-C single bonds, 7 C-O bonds, 7 C-H bonds, and 5 O-H bonds with average bond energies of 348 kJ/mol, 360 kJ/mol, 412 kJ/mol, and 463 kJ/mol respectively. The bond energy for C=O is 799 kJ/mol and O=O is 498 kJ/mol. The molar mass of fructose is 180.12 g/mol. Estimate the change in enthalpy if 2.56 g of fructose undergoes complete combustion at standard temperature and pressure.
Based on the bond energies for the reaction below, what is the enthalpy of the reaction? HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (g)
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