The reaction of nitrogen monoxide with ozone to produce nitrogen dioxide, is sho

Question

The reaction of nitrogen monoxide with ozone to produce nitrogen dioxide, is shown below NO(g)+O N2 (2)+02(g) The rate constants were measured at 25°C and 40°C and found to be 1.8x10* and 14x10 respectively, what is the activati on energy for this reaction? Select one O a. 1.3 x 104 J-Mol 1 o O b. 3.1 x 102 J Mol- c. 1.3x 10-4 J.Mol-1 O d. 3.1 x 10-4 J Mol The activation energy, E, can be defined as: Select one O a. The difference between the energy of the reactants and the energy of the products. O b. The difference between the energy of the activated complex and the energy of the products O c. The sum of the enthalpy change for the reaction and the energy of the activation complex O d. The difference between the energy of the reactants and the activated complex. The following reaction was observed in aqueous solution: 2Cu2*(aq)+ 6CN (aq) - 2Cu(CN)2(a)+(CN)2(aq). If the first step is the rapid development of Cu(CN)3 and the reaction rate was found to be kiCu2 ICN-1s, what is the rate-determining step of this reaction? Select one a. Cu(CN)2-(aq) O b. Cu(CN)3 (ag) O c. 2Cu(CN)2 (aq) O d. 2Cu(CN)3 (aq) Cu(CN)2-(aq) + (CN)2(aq) Cu(CN)2 (aq)+ (CN)a(ag) 2Cu(CN)2"(aq) + (CN)2(aq) 2Cu(CN)2-(aq) + (CN)2(aq)

Explanation / Answer

1)

Given:

T1 = 25 oC

=(25+273)K

= 298 K

T2 = 40 oC

=(40+273)K

= 313 K

K1 = 1.8*10^-14

K2 = 1.4*10^-14

use:

ln(K2/K1) = (Ea/R)*(1/T1 - 1/T2)

ln(1.4*10^-14/1.8*10^-14) = ( Ea/8.314)*(1/298.0 - 1/313.0)

-0.2513 = (Ea/8.314)*(1.608*10^-4)

Ea = -1.3*10^4 J/mol

Ea = -13 KJ/mol

Answer: a

2)

Ea = energy difference between activated complex and reactant

Answer: d

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