We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
determine delta H for Cl(g) + O3(g) —> ClO(g) +O2(g) 2 O3(g) -> 3 O2(g). H=-29.90...
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 = ????
The destruction of the ozone layer by chlorofluorocarbons (CFC’s) can be described by the following reactions: ClO(g) + O3(g) ? Cl(g) + 2 O2(g) ?H°rxn = –29.90 kJ 2 O3(g) ? 3 O2(g) ?H°rxn = 24.18 kJ Determine the value of heat of reaction for the following: Cl(g) + O3(g) ? ClO(g) + O2(g) ?H°=?
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
1. A 25 grams piece of unknown metal at 80 ºC is dropped into 50 grams of water at 25.0 ºC. The final temperature of the water is 26.16 ºC. What is the specific heat of the unknown metal? [Report answer to two sig figs and do not add the unit label.] 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)...
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
Assume the reaction 3 O2(g) <===> 2 O3(g) (Delta H° =285 kJ/mol) is at equilibrium. What effect will each of the following have (explain each)? a) adding more O2 b) adding more O3 c) removing O3 d) increasing pressure in the container e) adding an inert gas f) increasing the temperature in the container
(background info) Please explain how answer is achieved, it is -6.3 kj. (b) Assuming unlimited O2(e), what is the AH for this reaction when 6.0 grams of ClO react with O2? (4pts) 1. (a) Use the given thermochemical equations to calculate the standard enthalpy of reaction for the following equation: (Clear and complete work must be shown to receive full credit; 6 pts) Cle) + O3(e) → ClO(g) + O2(8). ClO(g) + O3(3) - Cl(g) + 2 O2(8) 2 03(8)...
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.
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
NO + O3--->NO2+O3 find delta rxn H, delta rxn S, and delta rxn G. for this reaction A=7.9x10^11cm^3/mole-s and Ea =10.5 KJ/mol. find delta H,delta S, delta G++ for this reaction. draw a reaction coordinate diagram for this reaction scaled correctly. Temperature of 293.13