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 the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(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
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. 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 = ????
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
Determine the equilibrium constant for the following reaction at 298 K: SO3(g) + H2O(g) → H2SO4(l) ΔG°rxn = -90.5 kJ mol-1 Group of answer choices 0.964 4.78 × 1011 7.31 × 1015 1.37 × 10-16 9.11 × 10-8
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
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.20 atm, P(O3) = 0.038 atm kj = ?
If the equilibrium constant for a one-electron redox reaction at 298 K is 7.9×104, calculate the corresponding ΔG∘ and E∘cell. A. ΔG∘= ? kJ B. E∘cell= ? V Please explain this problem to me. Thanks.
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.41 atm, P(O3) = 5.2 atm
Calculate the equilibrium concentrations of H2O, Cl, HCl, and O2 at 298 K if the initial concentrations are (H2O) = 0.070 M and (Cl2] = 0.120 M. The equilibrium constant Kc for the reaction H2O(g) + Cl2(g) + 2HCl(g) + O2(g) is 8.96 x 10 -9 at 298 K