CHAPTER 2
LITERATURE REVIEW
2.1 INTRODUCTION
Absorption column is an industrial column that being used to separate solute in the gas and to be absorbed by a liquid. Absorption column is frequently being used in processing of materials, purification and others activities. To ensure smooth and efficient operation, absorption column need to be designed for specific activities (McMahon & Osborne, 2013). A major application of absorption technology is by absorption in solutions of amine or alkaline salts for the removal of CO2 and H2S from natural gas or synthesis gas. Other than that, absorption column can be used to wash ammonia from a mixture of ammonia and air by using water.
McCabe et al. (2005) define absorption process occur when the
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Disadvantage of this column is liquid hydrostatic head caused high pressure drop.
Gas and Liquid flow rate
As stated by McCabe et al. (2005), the first task in designing absorption control system is to determine the flow rates and composition of each stream entering the column. From the law of conservation of mass, any material entering a process must either accumulate or exit, or in simple word, whatever comes in must go out. By using material balance, the flow rates and its composition can be determined.
Material balance for the control surface section of the column as shown by the dashed line in Figure 5, are as follows:
Total material balance: L_a+V=L+V_a (2.1)
Component A balance: L_a x_a+Vy=Lx+V_a y_a (2.2)
Where; V – Molar flow rate of gas phase L – Molar flow rate at liquid phase x – Liquid composition y – Gas composition
The overall material balance equations for the column are
Total material balance: L_a+V_b=L_b+V_a (2.3)
Component A balance: L_a x_a+V_b y_b=L_b x_b+V_a y_a
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The equilibrium lines are straight when solute concentrations are very dilute. Some of the restrictions of using Henry’s law are that it does not true for gases that react or dissociate upon dissolution.
Rate of Absorption and Mass Transfer Coefficients
The rate of absorption can be expressed by using individual or overall coefficients based on the liquid and gas phase. The rate of absorption can be expressed as r=k_y a(y-y_i ) (2.9) r=k_x a (x_i-x) (2.10) r=K_y a(y-y^*) (2.11) r=K_x a(x^*-x) (2.12)
The partial pressure difference (p – pi) can be used as driving force for gas phase as it is proportional to (y – yi). Diagrams based on the mole ratios Y and X are sometimes used as the operating line is straight. However, it is not recommended because ΔY and ΔX are not valid for measuring drive
Next, about 10 mL of both solutions, Red 40 and Blue 1, were added to a small beaker. The concentration of the stock solution were recorded, 52.1 ppm for Red 40 and 16.6 ppm for Blue 1. Then, using the volumetric pipette, 5 mL of each solution was transferred into a 10 mL volumetric flask, labelled either R1 or B1. Deionized water was added into the flask using a pipette until the solution level reached a line which indicated 10 mL. A cap for the flask was inserted and the flask was invented a few times to completely mix the solution. Then, the volumetric pipette was rinsed with fresh deionized water and
Using FIT with theses adjusted patterns I feel confident that I will complete this assignment
There is a 28,984% change from the mock up tank and the original. If you were to take a cross section parallel to the base of one of the holding tanks, how would you describe the shape? I would describe the shape as a sphere because a cross section is the same as the base. Samples of the tank's water are taken daily to ensure the salt density is correct to maintain aquatic life.
a. At 60 mm Hg, the data values in the table are not consistent with the data in the plots; for example, total mm Hg O2 bound is 30 with oxygen for Bonnie and 2 for Clyde. On the conventional plot, the 60 mm Hg is depicted at 50 with oxygen for Bonnie and about 9 for Clyde. The table says Bonnie should be shown at 6 instead of 19 at this concentration on the seating plot; also, the table says Clyde should be shown at 0 additional amount bound instead of 10 on the seating plot. b.
Now we place into the Erlenmeyer flask filled with Na2SO3 (aq), 30ml of 0.3 mol/L solution of HCl. 6. Right after mixing the two solutions, we quickly put the cap on the flask so that all of the gas produced is transferred through the glass tubes into the measuring cylinder. 7.
The dehydration of 2-methylcyclohexanol takes place at the bottom of the Hickman still. As the Hickman still heats up within the sand bath, the products evaporate and travel higher up in the still where they condense into a liquid and fall within the collection ring, thus separating the product from the remaining water. Drierite (CaSO4) is also added as a drying agent to absorb any leftover water within the product. The purity of the product will then be analyzed with infrared spectroscopy, paying attention to OH peak if it is present. Chemical Reactions: Data and Observations: Material Volume Mol.
After all data was collected, the equation M1V1= M2V2 was used to determine the initial concentrations of each reagent in each run. [Note: The final volume (V2) for each run was 11.0 mL or 0.011 L]. Used the volumes and given molarity concentrations illustrated in Table 1 for M1 and V1. Below, Table 2 shows the finished initial concentrations for each reagent in each of the four
Introduction: In this assignment, I will be doing two experimentations on examining the impact of temperature on the Alka-Seltzer’s response time. The first experimentation that I will be doing involves some water that is room temperature. The second experimentation that I will be doing involves some water that is very hot. If I want to be able to figure out the impact of the temperature on water, I will have to document the time it will take for the Alka-Seltzer to go into solution.
Introduction During this lab, students observed that not all substances dissolve at the same rate. Many factors involved including the independent and dependent variables affect how distinct substances dissolve. Overall, the chemical reaction, “the amount of reactant that changes the product in a given time”, played an important part in this experiment, when proven how a substance can change into another element by either emitting or absorbing energy. (Tro, 2018).
Materials -pan -50ml graduated cylinder -hydrogen peroxide -air stopper -water Graphs data A time 12 drops 8 drops 0 0 0 30 0 0.5 60 0 1 90 0 1 120 0 1 150 0 1 180 0 1.5 210 0 1.5 240 0 1.5 270 0 1.5 300 1 1.5 330 2 1.5 360 2 1.5 390 3 1.5 420 3 1.5 450 3 2 480 3 2 510 3 2 540 4 2.5 570 4 2.5 600 5 2.5 Data B time cold warm 0 0 0 30 1 1 60 2 1 90 2 2 120 2 2 150 2 2 180 2 2 210 2.5 2 240 3 2 270 3 2 300 3 2 330 3 3 360 3.5 3 390 3.5 3 420 3.5 3 450 3
The overall purpose of this lab was to develop a lab procedure in order to separate and measure the mass of each containment obtained the provided sample. In addition, this experiment was conducted in order to provide the EPA with a plan to remove all contaminants from a heterogenous mixture which purifies the water, making it accessible for the society. Furthermore, the sample consisted of the following contaminants, sand, rock, wood, plastic, salt, water, and an unknown metal. When it came to separating the contaminants, the wood and plastic were taken out through the use of tweezers, while the rocks were separated by decanting the mixture of sand and rocks from the water.
Another variable of the experiment that was controlled was the time in which the agar cubes spent in the sulphuric acid. The time allowed calculation of the rate of diffusion. The size of the agar cubes was controlled by using a grid and scalpel to, as accurately as possible, cut the agar cubes into the appropriate sizes. The shape of the agar cubes was also controlled. In future, this could be experimented with to investigate how different shaped agar blocks affect surface area to volume ratio and hence the rate of
Fractional distillation columns may contain a metal sponge, or have glass projections inside the column in order to increase the amount of surface area that the vapour comes into contact with. This causes some of the vapour to condense while in the fractional distillation column. Consequently, it falls back into the liquid reservoir. However, when this liquid to the reservoir, it contains a higher ratio of the more volatile substance than it did originally. This is repeated numerous times in the fractional distillation column and each time the liquid vapourizes, the vapour increases in purity.
After the reaction is finished, the percentage composition of each element in the product can be found and used to calculate the empirical formula, which is the lowest whole number ratio