Chlorine is a catalytic pathway for the destruction of ozone. Show how the photodissociation of a molecule of C2F2C12 can destroy two molecules of ozone, 3.
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- The average bond enthalpies of the C¬F and C¬Cl bonds are 485 kJ/mol and 328 kJ/mol, respectively. Given the fact that O2, N2, and O in the upper atmosphere absorb most of the light with wavelengths shorter than 240 nm, would you expect the photodissociation of C ¬ F bonds to be significant in the lower atmosphere?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)Δ?∘rxn=−122.8 kJ (2)2O3(g)⟶3O2(g)Δ?∘rxn=−285.3 kJ (3)O3(g)+Cl(g)⟶ClO(g)+O2(g) Δ?∘rxn= ?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) CIO(g) + 0;(g) Cl(g) + 20,(g) AHxn = -122.8 kJ AHan = -285.3 kJ (2) 203(g) → 30,(g) (3) 0,(g) + Cl(g) → CIO(g) + 0,(g) AHn = ?
- 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) C10(g) + O₂(g) → Cl(g) +20₂(g) AH (2) 20,(g) →30₂(g) (3) 0₂(g) + Cl(g) → CIO(g) + O₂(g) Allis= = -122.8 kJ AH = -285.3 kJ AHin = ? kJThe 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= ?(1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)ΔHrxn°=−122.8 kJ(2)2O3(g)⟶3O2(g)ΔHrxn°=−285.3 kJ(3)O3(g)+Cl(g)⟶ClO(g)+O2(g) ΔHrxn°= ? ΔH∘rxn=ΔHrxn°=__________________________________________kJThe 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. CIO(g) + O3(g) -> Cl(g) +202(g) AHxn = -122.8 kJ (1) (2) 203(g) - - 302(g) AHxn=-285.3 kJ (3) 03(g) + Cl(g) - CIO(g) + O2(g) AHixn= ? AHixn= kJ
- 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) C10(g) + 0,(g) - (2) 20;(g) (3) 0,(g) + Cl(g) → ClO(g) + 0, (g) Cl(g) + 2 0,(g) AH³xn -122.8 kJ > = → 30,(g) AHixn = -285.3 kJ → ClO(g) + 0,(g) AHixn = ? kJ rxnThe 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)Δ?∘rxn=−122.8 kJ(2)2O3(g)⟶3O2(g)Δ?∘rxn=−285.3 kJ(3)O3(g)+Cl(g)⟶ClO(g)+O2(g) Δ?∘rxn= ?(1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)ΔHrxn°=−122.8 kJ(2)2O3(g)⟶3O2(g)ΔHrxn°=−285.3 kJ(3)O3(g)+Cl(g)⟶ClO(g)+O2(g) ΔHrxn°= ? Δ?∘rxn=ΔHrxn°=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) CIO(g) + 0,(g) → Cl(g) + 20,(g) AH;xn = –122.8 kJ (2) 20,(g) → 30,(g) 0,(g)+Cl(g) → CIO(g) + 0,(g) AHn = -285.3 kJ (3) AĦxn = ? AHixn = kJ
- (c) At low temperatures, reaction (3) is replaced by the following reaction forming a stable dimer of CIO, which itself is rapidly photolysed to form Cl atoms: CIO + CIO Cl₂O2 2C1 + O2 Describe briefly, in qualitative terms, the effect that this reaction will have on the observed rate of ozone destruction. Note that Ka[Cl2] is the rate at which photons are absorbed by Cl2, and is often referred to as la.What is incomplete combustion of fossil fuels? Why can this be a problem?Ozone dissociates into O2 molecule and O atom by absorbing 03, ultraviolet light: O3 + hv → 02 + O. 1.00 liter of air contains 0.25 ppm ozone at 22 ° C temperature and 748 mm Hg pressure. All in a liter of air How many joules of energy should be absorbed for ozone to decompose according to the above reaction? Each photon absorbed is It will be deemed to have decomposed the O3 molecule and the light has a wavelength of 254 nm. (h=6.626 X 10-34 J.s)