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Provide a short paragraph that relates the most essential elements of theory behind the Wittig reaction
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- 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°=__________________________________________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. 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= kJCaluclate change H for the reaction 4 NH3 (g) + 5 O2 (g) -> 4 NO (g) + 6 H2O (g).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 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)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 = kJOrganic chemistry:Difference between sn1 and SN2 reactions
- Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.The Haber process is the principal industrial route for converting nitrogen into ammonia: N21g2 + 3 H21g2 ¡ 2 NH31g2Calculate the standard emf of the Haber process at room temperature1) Use Hess's Law to determine AH for the following target reaction. 3 CO₂(g) + 4 H₂O(g) b) C3Hg(g) + 5 O₂(g) C(s) + O₂(g) -CO₂(g) 2 H₂(g) + O₂(g) 3 C(s) + 4 H₂(g) →→→ 2 H₂O(g) C3H8(g) AH = AH = ΔΗ ΔΗ = ??? -2043 kJ -393.5 kJ -483.6 kJ
