Question

Hydroxyl radicals react with and eliminate many atmospheric pollutants. However, the hydroxyl radical does not clean up everything. For example, chlorofluorocarbons - which destroy stratospheric ozone - are not attacked by the hydroxyl radical. Consider the hypothetical reaction by which the hydroxyl radical might react with a chlorofluorocarbon: OH(g)+CF2Cl2(g)-->HOF(g)+CFCl2(g)Use bond energies to explain why this reaction is improbable. Calculate \Delta Hrxn of this reaction.

Answer 1

Answer:

ΔHreaction = 263.15 kJ/mol

Explanation:

The reaction is as follow:

OH + CF₂Cl₂ → HOF + CFCl₂

You need to calculate the enthalpy of reaction and for this it is necessary to know the standard enthalpies for each of the compounds. These enthalpies are as follows and can be found in your textbook or on the Internet.

ΔHreaction = ∑ΔHproducts - ∑ΔHreactants

$delta(H)_{reaction} =((1*(-97.8)+(1*(-92))-((1*39)+(1*(-491.15))=263.15kJ/mol$

Answer 2

Bond energy is defined as the strength of the bond of chemical bonds or the required to break the bonds. The $\Delta \text H_{\text{rxn}}$ for the given reaction is  263.15 kJ/mol.

The given chemical reaction between chlorofluorocarbons and hydroxyl ions is:

OH + CF₂Cl₂ → HOF + CFCl₂

The enthalpies of each bond when summed will determine the overall  $\Delta \text H_{\text{rxn}}$ for reaction. It can be expressed as:

$\Delta \text H_{\text{rxn}}$ = $\sum \Delta \text H$$_{\text{products}}$ -  $\sum \Delta \text H$$_{\text{reactants}}$

Putting the values:

$\Delta \text H_{\text{rxn}}$  = [1 x (-97.8) + 1 x (-92)] - [1 x (39) + 1 x (-491.15)]

$\Delta \text H_{\text{rxn}}$  = 263.15 KJ/mol

Therefore, $\Delta \text H_{\text{rxn}}$  for the reaction is 263.15 KJ/mol.

To know more about bond energies, refer to the following link:

https://brainly.com/question/17514510