The formation of NOC1 from No in the presence of a large excess of chlorine is p
ID: 1072466 • Letter: T
Question
The formation of NOC1 from No in the presence of a large excess of chlorine is pseudo first order in NO. In an experimental study of the reaction, the partial pressure of NOC1 is found to increase from 0 to 100 Pa in 800 s with an initial no pressure of 500 Pa. Determine the rate constant of the reaction and the half-life of NO? A second-order reaction of the type A + B = P was carried out in a solution that was initially 0.060 mol L^-1 in both A and B. After 1.0 h the concentration of A had fallen to 0.020 mol L^-1. Calculate the rate constant, what is half-life of reactants? Molecules A and B are in chemical equilibrium through the isomerization reaction with k_1 = 1.0 x 10^13 e^-45000/rt s^-1 and k_-1 = 2.0 * 10^13 e^-ea/rt s^-1. The equilibrium constant is found to double when the temperature is raised from 25degree C to 250degree C. Find the activation energy, E_a, for the reverse reaction (all energies are expressed in Joules). Determine the enthalpy change of the reaction. The oxidation of nitric oxide (nitrogen monoxide, NO) has an overall reaction written as: The gas-phase reaction goes through the following elementary steps: Use the steady state approximation to derive the rate law for NO_2 formation in gas phase. A metal catalyst such as Pt can catalyze the oxidation of NO. The metal catalyzed NO oxidation goes through a Langmuir-Hinshelwood mechanism consists of the following elementary steps: Derive the rate law based on the Langmuir-Hinshelwood mechanism. Compare the rate laws obtained for gas-phase and surface-catalyzed NO oxidations and discuss the difference in the context of reaction mechanism. The exchange current density and the electron transfer coefficient for the reaction 2H^+ + 2e doubleheadarrow on nickel at 25 degree C arc 6.3 * 10^-6 A cm^-2 and 0.42, respectively. Determine at what current density to obtain an overpotential of 0.25_V according to the Butler-Volmert equation. What will be the overpotential at the same current density according to the equation?Explanation / Answer
1 a)
The balanced reaction is-
NO +1/2 Cl --->NOCl
The rate for the production of NOCl is: d [NOCl] /dt = K [NO]2
Where K is the pseudo rate constant and Cl2 is in large excess
Using the integrated rate law for the reaction
NOCl =kt [NO]02 /1+kt[NO]0
But for constant volume, the partial pressures are directly proportional to the molar concentrations, so we can use these directly in this expression:
P NOCl = KtP^2NO0/1KtPNO0
K = P NOCl/t (P^2NO0 – P NOCL P NO0
= 100Pa/800((500)^2 – 100 x 500)
= 100Pa/800 (200000)
= 6.25 x 10^-7 Pa-1s-1
The rate constant of the reaction = 6.25 x 10^-7 Pa-1s-1
b) Half-life of NO
t1/2 = (1/K)
= {ln 2}/K
= 0.693/K
0.693/6.25 x 10^-7 =1.1088 x 10^6 s
Convert 1.1088 x 10^6 s into hour
1.1088 x 10^6 /60 x 60 = 308 hrs
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.