Question

Sodium fluoroacetate (NaO₂C₂H₂F) is a common poison used in New Zealand to control invasive species, such as rats. It can be prepared by the substitution of a C-Cl bond in sodium chloroacetate (NaO₂C₂H₂Cl) for a C-F bond. What is the approximate enthalpy change for this substitution reaction on a 1.500 mole sample, based on the following bond energies?
C-Cl = 339.0 kJ/mol
C-F = 485.0 kJ/mol

Answer 1

Answer:

-219

Explanation:

1.5(339) - 1.5(485) = -219

Answer 2

The approximate enthalpy change for this substitution reaction is -219 kJ.

In the case of this substitution reaction, we need to find the enthalpy change when NaO₂C₂H₂Cl is converted to NaO₂C₂H₂F.

This reaction involves the breaking of the C-Cl bond and the formation of the C-F bond.

We have to subtract the bond energy of the C-F bond from that of the C-Cl bond and multiply by the number of moles involved.

So we will have;

ΔH= 1.500 mole [339.0  kJ/mol - 485.0 kJ/mol]

ΔH= -219 kJ

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