The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) ClO (g) + O3 (g) ⟶Cl (g) + 2O2 (g) ΔH∘rxn=-122.8 kJ (2) 2O3 (g) ⟶3O2 (g) ΔH∘rxn=-285.3 kJ (3) O3 (g) + Cl (g) ⟶ClO (g) + O2 (g) ΔH∘rxn=?

Question

Zack Bowman

Chemistry

22 September, 05:13

The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) ClO (g) + O3 (g) ⟶Cl (g) + 2O2 (g) ΔH∘rxn=-122.8 kJ (2) 2O3 (g) ⟶3O2 (g) ΔH∘rxn=-285.3 kJ (3) O3 (g) + Cl (g) ⟶ClO (g) + O2 (g) ΔH∘rxn=?

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Raymond · Answer 1

-162,5 kJ/mol

Explanation:

Cl (g) + 2O2 (g) - -> ClO (g) + O3 (g) ΔH = 122.8 kJ/mol (as we used the reaction in the opposite direction, it will turn the enthalpy from exothermic to endothermic)

2O3 (g) - -> 3O2 (g) ΔH = - 285.3 kJ/mol

Cl (g) + O2 (g) - -> ClO (g) + O3 (g) ΔH = 122.8 kJ

+ 2O3 (g) - -> 3O2 (g) ΔH = - 285.3 kJ

O3 (g) + Cl (g) - -> ClO (g) + 2O2 (g) ΔH = 122.8 + (-285.3) = - 162,5 kJ