One mechanism for the destruction of ozone in the upper atomosphere is:Step 1: O3 (g) + NO (g) → NO2 (g) + O2 (g) [slow]Step 2: NO2 (g) + O (g) → NO (g) + O2 (g) [fast](a) Write the balanced overall reaction with state symbols. (1 point)(b) For the uncatalysed reaction, the activation energy is 14.0 kJ. The activation energy for thesame reaction when catalysed is 11.9 kJ. What is the ratio of the rate constant for the catalysedreaction to that for the uncatalysed reaction at 25 °C? Assume that the frequency factor A is thesame for each reaction and R to be 8.314 J/mol.K. (2 points)(c) One of the concerns about the use of Freons (CCl2F2) is that they will migrate to the upperatmosphere where chlorine atoms can be generated by the following reaction:CCl2F2 (g) ℎ𝑣→ CF2Cl (g) + Cl (g)Page 2 of 3RestrictedChlorine atoms can act as a catalyst in the destruction of ozone. The activation energy for thereactionCl (g) + O3 (g) → ClO (g) + O2 (g)is 2.1 kJ. Which is the more effective catalyst (Cl or NO) for the destruction of ozone? Explain.(1 point)(d) Compare the efficiency of Cl atom and NO molecules (by calculating the ratio of 𝑘Cl𝑘NO), assumingthat the frequency factor A is the same for each reaction. Show all working. (2 points)

(a) The balanced overall reaction is obtained by adding the two given reactions:

O3 (g) + NO (g) → NO2 (g) + O2 (g) NO2 (g) + O (g) → NO (g) + O2 (g)

O3 (g) + O (g) → 2 O2 (g)

(b) The ratio of the rate constants for the catalysed and uncatalysed reactions can be calculated using the Arrhenius equation:

k = Ae^(-Ea/RT)

where k is the rate constant, A is the frequency factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.

The ratio of k for the catalysed reaction (kc) to k for the uncatalysed reaction (ku) is:

kc/ku = e^((Ea_u - Ea_c)/RT)

Substituting the given values:

kc/ku = e^((14.0 kJ - 11.9 kJ)/(8.314 J/mol.K * 298 K))

Convert the activation energies from kJ to J (1 kJ = 1000 J):

kc/ku = e^((2100 J - 1190 J)/(8.314 J/mol.K * 298 K))

Calculate the exponent:

kc/ku = e^(910 J / (8.314 J/mol.K * 298 K))

Calculate the ratio:

kc/ku = e^0.366 ≈ 1.44

(c) The more effective catalyst for the destruction of ozone is the one with the lower activation energy, because a lower activation energy means that the reaction can proceed more quickly. In this case, Cl is the more effective catalyst because its activation energy (2.1 kJ) is lower than that of NO (11.9 kJ).

(d) The efficiency of Cl and NO as catalysts can be compared by calculating the ratio of their rate constants, kCl/kNO. This can be done in the same way as in part (b), using the Arrhenius equation and the given activation energies. The calculation is:

kCl/kNO = e^((Ea_NO - Ea_Cl)/RT)

Substituting the given values:

kCl/kNO = e^((11.9 kJ - 2.1 kJ)/(8.314 J/mol.K * 298 K))

Convert the activation energies from kJ to J:

kCl/kNO = e^((1190 J - 210 J)/(8.314 J/mol.K * 298 K))

Calculate the exponent:

kCl/kNO = e^(980 J / (8.314 J/mol.K * 298 K))

Calculate the ratio:

kCl/kNO = e^1.18 ≈ 3.26

So, Cl is approximately 3.26 times more efficient as a catalyst for the destruction of ozone than NO.