Effects of Free Convective Flow Past an Oscillating Semi-Infinite Vertical Plate with Variable Mass Diffusion Under First Order Chemical Reaction
Dr. A.R. Vijayalakshmi1 and M.SelvaJayanthi2
1 Department of Applied Mathematics, Sri Venkateswara College of Engineering,
Sriperumbudur- 602105, INDIA
2 SKP Engineering College, Tiruvannamalai – 606611
†Corresponding Author Email: avijaya@svce.ac.in
ABSTRACT
In this paper, An inquiry work to study the follow through of free convective viscous incompressible movement past an oscillating semi-infinite vertical plate with variable mass diffusion inferior first order chemical Reaction. The dimensionless governing equations are solved by a conclusively fixed and fast gather implicit finite variation
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and V.M. Soundalgekar (1998) presented the case of Combined Free and forced convection flow of water from a vertical plate with variable temperature. Unsteady MHD Convective Heat and Mass Transfer past a Semi-infinite vertical permeable Moving plate with Heat Absorption by Chamkha (2004). Effects of mass transfer on the flow an oscillating infinite vertical plate with constant heat flux have been studied by Soundalgekar et.al (1994). The effect on the flow past a vertical oscillating plate due to a combination of concentration and temperature differences was studied extensively by Soundalgekar and Akolkar (1983). During such chemical reactions, there is always a generation of heat. But when the foreign mass present in the fluid at very low level, we can assume a first- order chemical reaction and the heat generated due to the chemical reaction can be very negligible. Apelblat A (1980) studied analytical solution for Mass transfer with a chemical reaction of the first order. Chamber and Young have analyzed a first order chemical reaction in the neighborhood of a horizontal plate. Das, U.N, Ray, S.N, and Soundalgekar VM (2003).Mass transfer effects on flow past an impulsively started infinite vertical plate with constant mass flux –an exact solution. Ramamurthy and Govinda Rao (1971) presented the results for flow past an impulsively started infinite vertical plate. The effects of mass transfer on the transient free convection flow of a dissipative fluid …show more content…
The effects of the phase angles ω t on the average values of the skin-friction are shown Fig.11.lThe average skin-friction decreases with increasing phase angles ω t. The effects of the phase angles ω t, the chemical reaction parameter K on the average values of the Nusselet number are shown in Fig.12. Respectively. The average Nusselet number decreases with increasing phase angles ωt or increasing chemical reaction parameter.
5. CONCLUSION
The dimensionless governing equations are solved by an implicit scheme of Crank- Nicolson type. The carry out of velocity, temperature, concentration fields for different parameters are reviewed. The numerical solutions show that the number of time steps to reach steady – state depends powerfully on the chemical reaction parameter, velocity, temperature.
The principle Conclusions of the studies are as follows: 1. Velocity increasing with decreases Values of the chemical reaction parameters. 2. Concentration increases with decreasing chemical reaction parameter as well as Schmidt number. 3. Local as well as average skin-friction, Nusselet number, the Sherwood number increasing with increasing values of chemical reaction parameters. It is noticed that the improvement of mass diffusion to the buoyancy force increases the higher velocity
How is temperature related to this reaction? The higher the temperature the slower they move.
In “Searching the Flow Path,” P.J. Norwood and Sean Gray state that the American fire service dropping the ball on new tactics and the understanding of fire. Norwood and Gray point out that our enemy, fire, is not the same as it used to be. Additionally, the authors add that our training is preparing us well enough. They had that this lack of training is giving firefighters a false sense of security on the fireground. Undoubtedly, the authors believe that right hand/left hand search patterns are not the best option for today’s searches.
Abstract In this experiment, the reaction kinetics of the hydrolysis of t-butyl chloride, (CH3)3CCl, was studied. The experiment was to determine the rate constant of the reaction, as well as the effects of solvent composition on the rate of reaction. A 50/50 V/V isopropanol/water solvent mixture was prepared and 1cm3 of (CH3)3CCl was added. At specific instances, aliquots of the reaction mixture were withdrawn and quenched with acetone.
With many factors affecting chemical reactions, there is a significant relationship between these factors and the rate that they occur. As seen through many studies and experiments, surface area of solid reactants has a great impact on this rate of reaction. In conclusion, the scientist has learned important relationships and factors involved in the rate of which chemical reactions
A Cartesian Diver is and interesting science experiment that expresses the principles of Buoyancy, and the gas law known as “Boyles Law”. It is simply a 2 liter bottle that is filled with water, and has a Plastic Pipet with a brass nut attached to it. It is an easy, and fun way to demonstrate Buoyancy and the concepts of Chemistry to students. The Cartesian diver was named for the French philosopher and scientist René Descartes, who invented this marvelous experiment. The main science behind this experiment is Density.
Both substances reached a plateau and stopped diffusing after a certain number of minutes, which
The chemical equation that causes this to occur is: (2) The rate law is the relationship between the rate of a reaction and the concentrations of reactants.(3) In order to find the rate law the following equations must be used: Equation 1: Used to find the iodine concentration rate for each reaction. ([I])/t×〖10〗^5 Where [I] is the concentration of Iodine (moles/L) and t is the time in seconds taken for the iodine to completely disappear during the reaction. Equation 2: Used to find the concentration orders for acetone, hydrochloric acid and iodine.
Dependent The time taken for the bluish -black color to fade away (color of Iodine solution mix with starch solution ). The rate of enzyme reaction Minutes (min) Table 1.1 – Table shows the controlled variables in the experiment variables Units Measures of controlled variables.
Use these results to determine the product concentration, using Beer-Lambert’s Law: A= ɛCl (where A is the absorbance, ɛ is the molar absorptivity, C is the product concentration and l is the length of solution that the light passes through). Calculate the product concentrations at every minute for 10 minutes for all 7 of the test tubes using Beer-Lambert’s Law. Plot a graph of product concentration vs. time and then use the gradients of the 7 test tubes to determine the velocities of the reaction. After calculating the velocities, plot a Michaelis-Menten graph of velocity vs. substrate concentration.
Von Mises [3] states that “the forces due to viscosity appear as products of μ and expressions that have the dimensions area times (velocity / length)”. By further investigation, the mathematical analysis of these principles leads to a system of partial derivatives known as the Navier-Stokes equations. These equations are used to describe fluid flow and can be used to solve specific dynamic fluid flow cases. These include; velocities, pressure, temperature, density and can also be used to solve viscous problems of a dynamic fluid flow problems. These partial derivative equations relating to the specific variables are extremely complex and time-consuming to
What factors seem to cause a small coefficient of friction? Explain. Ans. Objects that tend to weigh less move more easily, so if in this experiment we put a marble instead of the weight. The marble would move quickly with a lower angle thus causing a small coefficient of friction.
Aim: To find out the relationship between the greater concentration of sodium thiosulfate when mixed with hydrochloric acid and the time it takes for the reaction (the time it takes for the solution to turn cloudy) to take place and to show the effect on the rate of reaction when the concentration of one of the reactants change. Introduction: The theory of this experiment is that sodium thiosulfate and hydrochloric acid reach together to produce sulfur as one of its products. Sulfur is a yellow precipitate so, the solution will turn to yellow color while the reaction is occurring and it will continue until it will slowly turn completely opaque. The reaction of the experiment happens with this formula: “Na2 S2 O3 + HCL =
The gradient gave the value of K, the rate constant for the reaction. Figure 2 shows the plotted graph Figure 2. From the
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.