The reaction 2NOCl rightarrow 2 NO + Cl2 has k = 9.3 times 10-5 L mol-1s-1 at 10
ID: 889163 • Letter: T
Question
The reaction 2NOCl rightarrow 2 NO + Cl2 has k = 9.3 times 10-5 L mol-1s-1 at 100 degree C and an activation energy of 99 kJ/mol. What is the rate constant at 130 degree C? At what temperature (Celsius) will the rate constant be 5.1 times 10-7 L mol-1 s-1? The figure below shows a potential energy diagram for a chemical reaction that can occur by two different reaction pathways. What is the equation for the overall reaction? What is the mechanism for the reaction with the higher pathway? What is the mechanism for the reaction with the lower pathway? On the figure, identify. 1) The activation energy for the reaction with the higher energy pathway, 2) the activation energy for the reaction with the lower energy path, and 3) Delta H for this reaction. Identify each of the species A to F as a reactant, intermediate, product, or catalyst.Explanation / Answer
2 NOCl ------> 2NO + Cl2
k1 = 9.3 x 10^-5 L mol^-1 s^-1
T1 = 100 degreeC = 373 K
Ea = 99 kJ/mol = 99 x 10^3 J/mol
(a) T2 = 130 degreeC = 403 K
log(k2/k1) = Ea / 2.303R ( 1/T1 - 1/T2)
log(k2 / 9.3 x 10^-5) = 99 x 10^3 / (2.303 * 8.314 ) ( 1 / 373 - 1 / 403)
log(k2 / 9.3 x 10^-5) = 1.032
k2 = 9.3 x 10^-5 * 10.76
k2 = 1 x 10^-3 L mol^-1 s^-1
(b)
k2 = 5.1 x 10^-7 L mol^-1 s^-1
log(k2/k1) = Ea / 2.303R ( 1/T1 - 1/T2)
log( 9.3 x 10^-5 / 5.1 x 10^-7) = 99 x 10^3 / ( 2.303 * 8.314) ( 1/373 - 1/T2)
2.261 = 5170.48 * ( 0.0027 - 1/T2)
4.37 x 10^-4 = 0.0027 - 1/T2
1/T2 = 2.27 x 10^-3
T2 = 441.95 K
T2 = 168.95 degreeC
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