1.) What is the transition state in the following reaction?
Cl + O3 ⟶ ClO + O2
ClO + O ⟶Cl + O2
O3 + O ⟶2O2 (overall reaction)
A) Cl
B) O3
C) O
D) ClO
E) O2
2.) What is the catalyst in the following reaction?
Cl + O3 ⟶ClO + O2
ClO + O ⟶Cl + O2
O3 + O ⟶2O2 (overall reaction)
A) Cl
B) O3
C) O
D) ClO
E) O2
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1.) What is the transition state in the following reaction? Cl + O3 ⟶ ClO +...
What is O3, O2, and O Step1: Cl + O3 ⇄ ClO + O2 Step2: ClO + O ⇄ Cl + O2 Total: O3 + O ⇄ 2O2 a. Cl(catalyst) b. O3 c. ClO(intermediate) d. O2 e. O
Identify the catalyst and intermediate in the following multi-step mechanism: step 1: Br+O3 -> BrO+ O2 step 2: BrO + O3 -> Br +2O2 a. There is no catalyst or intermediate in the above reaction b. Catalyst: O2 Intermediate: O3 c. Catalyst: BrO∙ Intermediate: Br∙ d. Catalyst: O3 Intermediate: O2 e. Catalyst: Br∙ Intermediate BrO
2. Determine the ∆H º for the third reaction; is it exothermic ? ClO(g) + O3(g) --> Cl(g) + 2 O2(g) ∆Hº = -29.90 kJ/mol 2 O3(g) --> 3 O2(g) ∆Hº = +24.18 kJ/mol Cl(g) + O3(g) --> ClO(g) + O2(g) ∆Hº = ????
One of the components of smog is ozone,O3, a colorless, toxic gas. It is a very strong oxidizing agent and causes respiratory illnesses. Ozone is produced in the lower atmosphere due to the catalytic effect of nitric oxide, NO, a byproduct of the combustion process in car engines. However, in the upper atmosphere ozone is a very useful gas, because it absorbs ultraviolet radiation and protects the earth from this high energy, damaging radiation. It is referred to as the...
Use Hess?s law to calculate ?G°rxn using the following information. ClO(g) + O3(g) ? Cl(g) + 2 O2(g) ?G°rxn = ? 2 O3(g)? 3 O2(g) ?G°rxn = +489.6 kJ Cl(g) + O3(g) ? ClO(g) + O2(g) ?G°rxn = -34.5 kJ
Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(g) + O2(g) ΔG° = - 34.5 kJ Please explain how you enter it into the calculator I get 1.23*10^-14. Which is incorrect the answer is 1.12*10^-6.
determine delta H for Cl(g) + O3(g) —> ClO(g) +O2(g) 2 O3(g) -> 3 O2(g). H=-29.90 kj/mol ClO(g) + O3(g) -> Cl(g) + 2 O2(g). H=+24.18 kj/mol report to 4 sigfigs
Reaction A $$O3(g)+Cl(g)ClO(g)+O2(g) $$A=2.93×10−11 cm3molecule • s and Ea=2.16 kJmol Reaction B $$O3(g)+NO(g)NO2(g)+O2(g) $$A=2.34×10−12 cm3molecule • s Ea=11.6 kJmol On the basis of the frequency factors and activation energy values above, calculate the rate constant for Reaction A at 298 K. On the basis of the frequency factors and activation energy values above, calculate the rate constant for Reaction B at 298 K. We were unable to transcribe this imageWe were unable to transcribe this image
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
1) 2) 3) C3H8(g) + 5 O2(g) = 3 CO2(g) + 4H2O(1) AH = -2220 kJ Decreasing the temperature will result in shift the equilibrium to the right shift the equilibrium to the left Keq is decreased O no effect in shifting the equilibrium more information is needed Which of the following expressions is the correct equilibrium-constant expression for the reaction below? P4010(s) = P4(s) + 5 O2(g) [02]-5 O [0215 [P4010] [Pd][02] [P][0215 O [P4010] [P4010) [P][0,1175 A proposed...