a) To deduce the orders of the reaction, we need to compare the experiments.
To find order with respect to NO, we will compare experiment 1 and 2, because the [O2] is same in both.
rate1/rate2 = ([NO]1/[NO]2)x
(2.1*10-7)/(1.9*10-6)= ((1.5*10-5)/(4.5*10-5) )x
0.11 = (0.33)x
Taking log on both sides
log 0.11 = x log 0.33
x = 2
So, order with respect to [NO] is 2.
Similarly, to find order with respect to O2, we will compare experiment 1 and 3, because the [NO] is same in both.
rate1/rate3 = ([O2]1/[O2]3)y
(2.1*10-7)/(8.4*10-7)= ((0.5*10-5)/(2.0*10-5) )y
0.25 = (0.25)y
y = 1
So, order with respect to [O2] is 1.
b) Rate equation =>
rate = k [NO]2[O2]1
For experiment 1:
rate = 2.1*10-7 mol cm-3 s-1
[NO] = 1.5*10-5 mol cm-3
[O2] = 0.5*10-5 mol cm-3
Put all these values in rate equation
2.1*10-7 = k (1.5*10-5)2(0.5*10-5)
k = 1.87*108 cm3 mol-1 s-1
c) When a reaction is actually occuring through a number of steps, then the slowest step of that reaction is the rate determining step. This means that the rate of the whole reaction will depend on that step.
d) There are two fundamental types of adsorption: physisorption and chemisorption. Physisorption occurs due to vander waal forces and chemisorption occurs due to chemical bonds. Out of these two, chemisorption formed monolayer and physisorption forms multilayers.
Nitrogen (II) oxide reacts with oxygen in the following reaction: Experiments were carried out to determine...
Question 11. Hydrogen reacts with nitrogen to form ammonia. This reaction has been studied in the laboratory, and the following rate data were determined at 25 °C 3H2 N 2NH Rate (mol L's) [H:l (mol/L) N (mol/L) Trial 1.00 x 10 4.00x 10 2.61x10 9.00x 10 2.00x 10 3.96 x 10 1.00 x 10 2.00 x 10 3 6.60 x 10 5.94 x10 3.00x 10 9.00x 10 4 Detemine the order of the reaction with respect to Nz gas (S...
Consider the following reaction carried out in liquid 2A+3B- Table Q1.1 lists the initial rate of reaction for the initial concentration of A and B Table Q1.1: Initial reaction rate, vo [mol/m'.s] (IC, 0.000 [mol/m') Initial concentration of A, [Al, [mol/m 10.00 20.00 50.00 316.23 Initial 28.28 20.00 89.44 1000.0 concentration 25.00 of B, 75.00 [Bl, [moVm'] In (a) Show the reaction rate of C, ve, by using krfvi, [4], [3] (6 marks) POI/CO1/C3) (b) Evaluate the rate constant, k,,...
From the data table determine the rate law for reactions 1-4
and calculate the value of k for each. Thanks
I-IV
BACKGROUND
INFORMATION
Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2
Concentration= 0.44 M
•Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M
•Calculation of I^- after mixing for parts I,II, IV= 0.10
M
•Calculation of Initial (mol/L-s)
Filled in Table
Now the solutions for Rate Order and Rate Constant are
needed
Reactants 8 ml 30% HO, 2...
What are the instruments that have been utilized for the
review article discussions?
`
1. Introduction In recent years, nanoclays have been the object of particular interest for many scientists and researchers in chemistry, physics, engineering and biology due to their excellent properties as well as their sustain- ability [1-3]. For instance, they represent the starting point to the de velopment of smart materials for drug delivery (4-9), food packaging [10-12), environmental remediation and wastewater treatment [13], cultural heritage [14–17and...
Based on the document below,
1. Describe the hypothesis Chaudhuri et al ids attempting to
evaluate; in other words, what is the goal of this paper? Why is he
writing it?
2. Does the data presented in the paper support the hypothesis
stated in the introduction? Explain.
3.According to Chaudhuri, what is the potential role of thew
alkaline phosphatase in the cleanup of industrial waste.
CHAUDHURI et al: KINETIC BEHAVIOUR OF CALF INTESTINAL ALP WITH PNPP 8.5, 9, 9.5, 10,...