An important reaction in the formation of photochemical smog is the reaction bet

Question

An important reaction in the formation of photochemical smog is the reaction between ozone and NO: No(g) + O_3(g) rightarrow NO_2 (g) + O_2(g) The reaction is first order in NO and O_3. The rate constant of the reaction is 80.0 M^-1 s^-1 at 25 degree C and 3.000 Times 10^3 M^-1 S^-1 at 75 degree C. Answer parts (a), (b), (c), and (d) below. If this reaction were to occur in a single step, would the rate law be consistent with the observed order of the reaction for NO and O_3? What is the value of the activation energy of the reaction? What is the rate of the reaction at 25 degree C when [NO] = 3.45 Times 10^-6 M and [O_3] = 5.03 Times 10^-9 M? Predict the values of the rate constant at the following temperatures:

Explanation / Answer

d)
Ea = 62488 J/mol (as calculated in part b)
T1 = 25 Oc = (273+25) = 298 K
K1 = 80 M-1s-1
T2 = 10 Oc = (273+10) K = 283 K
K2 = ?

usE:
ln (K2/K1) = Ea/R * (1/T1 - 1/T2)
ln (K2/80) = 62488/8.314 * (1/298 - 1/283)
ln (K2/80) = -1.337
K2/80 = 0.263
K2 = 21 M-1s-1

Answer: At 10 oC, K = 21 M-1s-1

-------------------------
Ea = 62488 J/mol (as calculated in part b)
T1 = 25 Oc = (273+25) = 298 K
K1 = 80 M-1s-1
T2 = 35 Oc = (273+35) K = 308 K
K2 = ?

usE:
ln (K2/K1) = Ea/R * (1/T1 - 1/T2)
ln (K2/80) = 62488/8.314 * (1/298 - 1/308)
ln (K2/80) = 0.819
K2/80 = 2.268
K2 = 181.4 M-1s-1

Answer: At 35 oC, K = 181.4 M-1s-1

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