Question 1

Use Hess's law to calculate ΔG°_rxn using the following information. CO(g)→ C(s)+ 1/2 O₂(g)ΔG°_rxn= ? CO₂(g)→ C(s)+ O₂(g)ΔG°_rxn= +394.4 kJ CO(g)+ 1/2 O₂(g)→ CO₂(g)ΔG°_rxn= -257.2 kJ

Accepted Answer

The answer of Use Hess's law to calculate ΔG°_rxn using...

Question 2

Choose the statement below that is true.

Accepted Answer

At equilibrium, the Gibbs free energy change (ΔG_rxn) is zero, indicating no net change in the system.

Question 3

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq)+ NO(g)→ 3 NO₂(g)+ H₂O(l)ΔG°_rxn= ? ΔH°_f (kJ/mol)-207.0 91.3 33.2 -285.8 S°(J/mol^∙K)46.0 210.8 240.1 70.0

Accepted Answer

The answer of Calculate the ΔG°_rxn using the following information. 2...

Question 4

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g)+ O₂(g)→ 2 HgO(s)ΔG° = -180.8 kJ P(Hg)= 0.025 atm,P(O₂)= 0.037 atm

Accepted Answer

First, we need to calculate the ΔG for the given reaction using the formula: ΔG = ΔG° + RT ln(Q) where ΔG° is the standard free energy change, R is the gas constant (8.314 J/K·mol), T is the temperature in Kelvin (298 K), and Q is the reaction quotient. Q can be calculated using the given partial pressures of Hg and O2: Q = (P(Hg))^2/ P(O₂) Q = (0.025 atm)^2/0.037 atm Q = 0.0169 atm Substituting values into the formula, we get: ΔG = -180.8 kJ + (8.314 J/K·mol × 298 K × ln(0.0169)) ΔG = -283.9 kJ/mol Finally, we can calculate the ΔG for the desired conditions using the formula: ΔG = ΔG° + RT ln(Q/P°) where P° is the standard state pressure (1 atm). For Hg and O2, we get: ΔG = -180.8 kJ + (8.314 J/K·mol × 298 K × ln(0.0169/1)^2) ΔG = -154.4 kJ/mol Therefore, the answer is B, which is the only option with a negative value. A negative ΔG indicates that the reaction is spontaneous under the given conditions.

Question 5

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. SO₃(g)+ H₂O(g)→ H₂SO₄(l)ΔG°= -90.5 kJ P(SO₃)= 0.20 atm,P(H₂O)= 0.88 atm

Accepted Answer

To calculate ΔG_rxn, use the equation ΔG = ΔG° + RT ln(Q), where Q is the reaction quotient. Here, Q = P(SO3) * P(H2O) = 0.20 * 0.88. Plugging in the values, ΔG = -90.5 kJ + (8.314 J/mol*K * 298 K * ln(0.176)) = -86.2 kJ.

Question 6

Calculate the ΔG°_rxn using the following information. 2 H₂S(g)+ 3 O₂(g)→ 2 SO₂(g)+ 2 H₂O(g)ΔG°_rxn= ? ΔG°_f (kJ/mol)-33.4 -3300.1 -228.6

Accepted Answer

The answer of Calculate the ΔG°_rxn using the following information. 2...

Question 7

Determine ΔG°_rxn using the following information. CaCO₃(s)→ CaO(s)+ CO₂(g)ΔH° = +179.2 kJ;ΔS° = +160.2 J/K

Accepted Answer

ΔG° = ΔH° - TΔS°. Assuming T = 298 K, ΔG° = 179.2 kJ - (298 K)(0.1602 kJ/K) = 131.4 kJ.

Question 8

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. CaCO₃(s)→ CaO(s)+ CO₂(g)ΔG° = +131.1 kJ P(CO₂)= 0.033 atm

Accepted Answer

We can use the equation ΔG = ΔG° + RTln(Q) where Q is the reaction quotient. At equilibrium, Q is equal to the equilibrium constant K. 
First, we need to calculate Q: 
Q = P(COS12)/P(CaO) 
Since CaO is a solid, its pressure is fixed at 1 atm. Thus, Q = 0.033 atm / 1 atm = 0.033. 
Next, we can substitute the given values into the equation: 
ΔG = +131.1 kJ + (8.314 J/K/mol)(298 K) * ln(0.033) 
ΔG = +122.6 kJ 
Therefore, the answer is C, which is the closest to +122.6 kJ.

Question 9

Determine ΔG°_rxn using the following information. FeO(s)+ CO(g)→ Fe(s)+ CO₂(g)ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Accepted Answer

ΔG° = ΔH° - TΔS°. Assuming standard temperature (298 K), ΔG° = (-11.0 kJ) - (298 K)(-17.4 J/K × 1 kJ/1000 J) = -11.0 kJ + 5.1852 kJ = -5.8 kJ.

Question 10

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g)+ 5 N₂H₄(l)→ 7 N₂(g)+ 12 H₂O(l)ΔG°_rxn= ? ΔH°_f (kJ/mol)-133.9 50.6 -285.8 S°(J/mol^∙K)266.9 121.2 191.6 70.0

Accepted Answer

- First, we need to calculate the standard entropy change ΔS°rxn using the equation:
ΔS°rxn = ΣS°(products) - ΣS°(reactants)
ΔS°rxn = [7(121.2) + 12(70.0)] - [4(266.9) + 5(191.6) + 14(70.0)]
ΔS°rxn = -442.6 J/K
- Next, we need to calculate the standard enthalpy change ΔH°rxn using the given values of standard enthalpies of formation:
ΔH°rxn = [7(0) + 12(-285.8)] - [4(-133.9) + 5(50.6) + 14(0)]
ΔH°rxn = -4167.8 kJ/mol
- Finally, we can calculate the standard Gibbs free energy change ΔG°rxn using the equation:
ΔG°rxn = ΔH°rxn - TΔS°rxn
We need to convert the units of ΔS°rxn to kJ/mol before plugging in the values:
ΔG°rxn = -4167.8 kJ/mol - (298 K)(-0.4426 kJ/mol/K)
ΔG°rxn = -3297.9 kJ/mol
Rounding to three significant figures, we get:
ΔG°rxn = -3.298 × 10³ kJ/mol, which corresponds to answer choice E.

Question 11

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g)+ O(g)→ NO₂(g)ΔG°_rxn= ? 2 O₃(g)→ 3 O₂(g)ΔG°_rxn= +489.6 kJ O₂(g)→ 2 O(g)ΔG°_rxn= +463.4 kJ NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)ΔG°_rxn= -199.5 kJ

Accepted Answer

We can use Hess's law to calculate the overall ΔG°_rxn by summing the ΔG°_rxn values for each step in the reaction: 1. NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔG°_rxn= -199.5 kJ (given) 2. O₂(g) → 2 O(g) ΔG°_rxn= +463.4 kJ (given) 3. 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ (given, but reversed in order to match reaction 1) Adding these three reactions and their respective ΔG°_rxn values gives: NO(g) + 2O₃(g) → NO₂(g) + 3O(g) ΔG°_rxn= -199.5 kJ + (+463.4 kJ) + (-489.6 kJ) ΔG°_rxn= -225.7 kJ Therefore, the best answer choice is C, -676.0 kJ. However, this answer is not provided in the choices, so the closest choice is A, +753.5 kJ, which is the reverse of the correct answer.

Question 12

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq)+ NO(g)→ 3 NO₂(g)+ H₂O(l)ΔG°_rxn= ? ΔG°_f (kJ/mol)-110.9 87.6 51.3 -237.1

Accepted Answer

The answer of Calculate the ΔG°_rxn using the following information. 2...

Question 13

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g)+ 5 N₂H₄(l)→ 7 N₂(g)+ 12 H₂O(l)ΔG°_rxn= ? ΔG°_f (kJ/mol)-73.5 149.3 -237.1

Accepted Answer

The correct answer is A because the ΔG°_rxn can be calculated using the formula:ΔG°_rxn = ΣΔG°_f(products) - ΣΔG°_f(reactants)ΔG°_rxn = [7ΔG°_f(N₂) + 12ΔG°_f(H₂O)] - [4ΔG°_f(HNO₃) + 5ΔG°_f(N₂H₄)]ΔG°_rxn = [7(-237.1 kJ/mol) + 12(0 kJ/mol)] - [4(-73.5 kJ/mol) + 5(149.3 kJ/mol)]ΔG°_rxn = -3.298 × 10³ kJ

Question 14

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. Fe₂O₃(s)+ 3 CO(g)→ 2 Fe(s)+ 3 CO₂(g)ΔG° = -28.0 kJ P(CO)= 1.4 atm,P(CO₂)= 2.1 atm

Accepted Answer

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Question 15

Choose the statement below that is true.

Accepted Answer

If the equilibrium constant, K, is less than 1, it means that the concentration of products is smaller than the concentration of reactants. Hence, the backward reaction will be spontaneous in order to reach the equilibrium constant. Therefore, choice A is true.

Question 16

Determine ΔG°_rxn using the following information. H₂(g)+ CO(g)→ CH₂O(g)ΔH° = +1.9 kJ;ΔS° = -109.6 J/K

Accepted Answer

The answer of Determine ΔG°_rxn using the following information. H₂(g)+ CO(g)→...

Question 17

Calculate the ΔG°_rxn using the following information. 2 H₂S(g)+ 3 O₂(g)→ 2 SO₂(g)+ 2 H₂O(g)ΔG°_rxn= ? ΔH°_f (kJ/mol)-20.6 296.8 -241.8 S°(J/mol^∙K)205.8 205.248.2 188.8

Accepted Answer

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Question 18

Which of the following is not true for ΔG_rxn?

Accepted Answer

The answer of Which of the following is not true...

Question 19

Calculate ΔG_rxn 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

Accepted Answer

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Question 20

Use Hess's law to calculate ΔG°_rxn using the following information. ClO(g)+ O₃(g)→ Cl(g)+ 2 O₂(g)ΔG°_rxn= ? 2 O₃(g)→ 3 O₂(g)ΔG°_rxn= +489.6 kJ Cl(g)+ O₃(g)→ ClO(g)+ O₂(g)ΔG°_rxn= -34.5 kJ

Accepted Answer

The answer of Use Hess's law to calculate ΔG°_rxn using...

Quiz 17: Free Energy and Thermodynamics

Use Hess's law to calculate ΔG°_rxn using the following information. CO(g) → C(s) + 1/2 O₂(g) ΔG°_rxn= ? CO₂(g) → C(s) + O₂(g) ΔG°_rxn= +394.4 kJ CO(g) + 1/2 O₂(g) → CO₂(g) ΔG°_rxn= -257.2 kJ

Choose the statement below that is true.

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol^∙K) 46.0 210.8 240.1 70.0

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O₂) = 0.037 atm

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. SO₃(g) + H₂O(g) → H₂SO₄(l) ΔG°= -90.5 kJ P(SO₃) = 0.20 atm,P(H₂O) = 0.88 atm

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔG°_f (kJ/mol) -33.4 -3300.1 -228.6

Determine ΔG°_rxn using the following information. CaCO₃(s) → CaO(s) + CO₂(g) ΔH° = +179.2 kJ;ΔS° = +160.2 J/K

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. CaCO₃(s) → CaO(s) + CO₂(g) ΔG° = +131.1 kJ P(CO₂) = 0.033 atm

Determine ΔG°_rxn using the following information. FeO(s) + CO(g) → Fe(s) + CO₂(g) ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol^∙K) 266.9 121.2 191.6 70.0

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g) + O(g) → NO₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ O₂(g) → 2 O(g) ΔG°_rxn= +463.4 kJ NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔG°_rxn= -199.5 kJ

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -110.9 87.6 51.3 -237.1

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -73.5 149.3 -237.1

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm,P(CO₂) = 2.1 atm

Choose the statement below that is true.

Determine ΔG°_rxn using the following information. H₂(g) + CO(g) → CH₂O(g) ΔH° = +1.9 kJ;ΔS° = -109.6 J/K

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔH°_f (kJ/mol) -20.6 296.8 -241.8 S°(J/mol^∙K) 205.8 205.248.2 188.8

Which of the following is not true for ΔG_rxn?

Calculate ΔG_rxn 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

Use Hess's law to calculate ΔG°_rxn using the following information. ClO(g) + O₃(g) → Cl(g) + 2 O₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ Cl(g) + O₃(g) → ClO(g) + O₂(g) ΔG°_rxn= -34.5 kJ

Quiz 17: Free Energy and Thermodynamics

Use Hess's law to calculate ΔG°rxn using the following information. CO(g) → C(s) + 1/2 O2(g) ΔG°rxn = ? CO2(g) → C(s) + O2(g) ΔG°rxn = +394.4 kJ CO(g) + 1/2 O2(g) → CO2(g) ΔG°rxn = -257.2 kJ

Choose the statement below that is true.

Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K) 46.0 210.8 240.1 70.0

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O2) = 0.037 atm

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. SO3(g) + H2O(g) → H2SO4(l) ΔG°= -90.5 kJ P(SO3) = 0.20 atm,P(H2O) = 0.88 atm

Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔG°rxn = ? ΔG°f (kJ/mol) -33.4 -3300.1 -228.6

Determine ΔG°rxn using the following information. CaCO3(s) → CaO(s) + CO2(g) ΔH° = +179.2 kJ;ΔS° = +160.2 J/K

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. CaCO3(s) → CaO(s) + CO2(g) ΔG° = +131.1 kJ P(CO2) = 0.033 atm

Determine ΔG°rxn using the following information. FeO(s) + CO(g) → Fe(s) + CO2(g) ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol∙K) 266.9 121.2 191.6 70.0

Use Hess's law to calculate ΔG°rxn using the following information. NO(g) + O(g) → NO2(g) ΔG°rxn = ? 2 O3(g) → 3 O2(g) ΔG°rxn = +489.6 kJ O2(g) → 2 O(g) ΔG°rxn = +463.4 kJ NO(g) + O3(g) → NO2(g) + O2(g) ΔG°rxn = -199.5 kJ

Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1

Calculate the ΔG°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -73.5 149.3 -237.1

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm,P(CO2) = 2.1 atm

Choose the statement below that is true.

Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH° = +1.9 kJ;ΔS° = -109.6 J/K

Calculate the ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔG°rxn = ? ΔH°f (kJ/mol) -20.6 296.8 -241.8 S°(J/mol∙K) 205.8 205.248.2 188.8

Which of the following is not true for ΔGrxn?

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

Use Hess's law to calculate ΔG°rxn using the following information. ClO(g) + O3(g) → Cl(g) + 2 O2(g) ΔG°rxn = ? 2 O3(g) → 3 O2(g) ΔG°rxn = +489.6 kJ Cl(g) + O3(g) → ClO(g) + O2(g) ΔG°rxn = -34.5 kJ

Use Hess's law to calculate ΔG°_rxn using the following information. CO(g) → C(s) + 1/2 O₂(g) ΔG°_rxn= ? CO₂(g) → C(s) + O₂(g) ΔG°_rxn= +394.4 kJ CO(g) + 1/2 O₂(g) → CO₂(g) ΔG°_rxn= -257.2 kJ

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol^∙K) 46.0 210.8 240.1 70.0

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O₂(g) → 2 HgO(s) ΔG° = -180.8 kJ P(Hg) = 0.025 atm,P(O₂) = 0.037 atm

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. SO₃(g) + H₂O(g) → H₂SO₄(l) ΔG°= -90.5 kJ P(SO₃) = 0.20 atm,P(H₂O) = 0.88 atm

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔG°_f (kJ/mol) -33.4 -3300.1 -228.6

Determine ΔG°_rxn using the following information. CaCO₃(s) → CaO(s) + CO₂(g) ΔH° = +179.2 kJ;ΔS° = +160.2 J/K

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. CaCO₃(s) → CaO(s) + CO₂(g) ΔG° = +131.1 kJ P(CO₂) = 0.033 atm

Determine ΔG°_rxn using the following information. FeO(s) + CO(g) → Fe(s) + CO₂(g) ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔH°_f (kJ/mol) -133.9 50.6 -285.8 S°(J/mol^∙K) 266.9 121.2 191.6 70.0

Use Hess's law to calculate ΔG°_rxn using the following information. NO(g) + O(g) → NO₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ O₂(g) → 2 O(g) ΔG°_rxn= +463.4 kJ NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔG°_rxn= -199.5 kJ

Calculate the ΔG°_rxn using the following information. 2 HNO₃(aq) + NO(g) → 3 NO₂(g) + H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -110.9 87.6 51.3 -237.1

Calculate the ΔG°_rxn using the following information. 4 HNO₃(g) + 5 N₂H₄(l) → 7 N₂(g) + 12 H₂O(l) ΔG°_rxn= ? ΔG°_f (kJ/mol) -73.5 149.3 -237.1

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm,P(CO₂) = 2.1 atm

Determine ΔG°_rxn using the following information. H₂(g) + CO(g) → CH₂O(g) ΔH° = +1.9 kJ;ΔS° = -109.6 J/K

Calculate the ΔG°_rxn using the following information. 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) ΔG°_rxn= ? ΔH°_f (kJ/mol) -20.6 296.8 -241.8 S°(J/mol^∙K) 205.8 205.248.2 188.8

Which of the following is not true for ΔG_rxn?

Calculate ΔG_rxn 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

Use Hess's law to calculate ΔG°_rxn using the following information. ClO(g) + O₃(g) → Cl(g) + 2 O₂(g) ΔG°_rxn= ? 2 O₃(g) → 3 O₂(g) ΔG°_rxn= +489.6 kJ Cl(g) + O₃(g) → ClO(g) + O₂(g) ΔG°_rxn= -34.5 kJ