Morphologies Of The As-Formed Zeolite Nannostructures Products

2. Does the rate of diffusion correspond with the molecular weight of the dye? The the density of the medium and the molecular weight of the dye will determine the rate of diffusion.

The concentrations and absorbances of the red and blue dyes were used to find the concentration of the purple dyes. From the graph of the blue dye, the linear equation for absorbance was y = mx + b. From that formula came the equation y = 7.915 x 104 (x) + 0.02489, where y represents absorbance, m is slope, x is concentration/molarity, and b is the constant/y-intercept. The same set up was performed for the red dye, but the equation produced was y = 1.045 x 104 (x) +.001298. The equations found when graphing absorbance vs. concentration were used to find the concentration of the purple dyes. The absorbance for purple dye 3 on the red wavelength of 470 nm equaled 0.149 and 0.818 for the blue wavelength of 635 nm. For purple dye 1

With these absorbance numbers a concentration curve was constructed and the unknown solution was determined by finding the point of absorbance on the curve.

Kinetics is the study of the rate of chemical processes. The kinetics of the reaction between crystal violet and NaOH was studied. In order to monitor crystal violet concentration as a function of time, a spectroscopic colorimeter was used. What is the rate law for decolorization of crystal violet? In order to figure this out, the rate of the reaction of crystal violet and sodium hydroxide must be found. In this experiment, the initial goals were to determine the overall rate law for the rate of decolorization of crystal violet in basic solutions as a function of time and to determine the rate law for the reaction including the actual value of k; Rate = k[A]x[B]y. The rate of a reaction was expected to depend on the concentrations

c) Choose “ln( )” from the function list as the formula for the column in the equation edit box. Next Select absorbance from the variable list. In the equation edit box, you should now displayed: ln (“absorbance”). Click Ok.

The values of color absorbance are effective because color absorbance has a linear relationship with concentration values, which in turn, allows us to easily find concentration values for many solutions. Beer’s law describes this phenomenon since the absorbance is directly proportional to concentration. We observed that as the color absorbance increased, the concentration of the FeSCN2+ complex ion increased. This is because as the FeSCN2+ concentration increases, the blood-red color becomes darker due to more presence of the blood-red FeSCN2+ ion. Therefore, the color absorbance increases because there is more blue color absorbed by the darker red color. We then graphed the absorbance and concentration values and created a line of best fit. Using the line of best fit, we were able to predict the equilibrium concentrations of the FeSCN2+ solutions and find the change required to reach equilibrium. Since we already knew the initial concentration of FeSCN2+ and since we already found the equilibrium concentration of FeSCN2+, we can calculate the change in equilibrium. Using this data, we were able to calculate the equilibrium concentration of all of the species in this lab, since we already knew the change from the initial concentration to the equilibrium change. Q is less than K because there was no initial concentration of FeSCN2+, but after the system reached

Fig1 shows on the right group one next to it, 1st half of our result on electrophroresis gel. The 2nd half for the gel is our experiment compared to Anderson group 6. The 1st layer in all 3 pictures is the bound dye, the 2nd layer is the free dye.

Figure 2: Dye percents versus absorbance in a control, 10%, 20%, and 30% azide solutions.

Looking at just the control data series, the absorbances decreased as the concentration of the dye increased. Looking at the data series that includes the sodium azide, the absorbances decreased as the concentration of the dye increased. Sodium azide blocks the electron flow of the electron transport chain, which means energy is not needed. ATP production depends on the electron transport chain. Passive transport is able to transport molecules across the membrane without energy. So passive transport is the only way the neutral red dye could be transported across the

Firstly, if we consider the data collected in tables from my primary and secondary evidence, we can see that the values of the range of diffusion reaction are higher when the concentration of food colouring dye used is higher in percentage. Specifically, when the concentration is at 0%, there is no diffusion reaction at all. In contrast, as we increase the percentage of food dye used by a specific set value (+20% each time) the distance (radius or diameter) of food dye formed from diffusion around the well becomes steeper.

You could be forgiven for thinking the word Zeolite is the name of the next Hollywood hero out to save the world, or an ancient Greek god. The reality is that when it comes to improving your vegetable garden, this fascinating mineral supplement is actually a bit of an organic superhero...

Based on Figure 4.6 the metals cations will enter into the pores of zeolite NaA and urged the metals alkali and alkaline earth cations which are soluble in water. In addition, zeolite NaA more selective towards the transition metals because it has larger sizes so easy dipolariasi (Auerbach, et al. 2003) Zeolite NaA tend to bind cations because the negatively charged zeolite cavities. The negative charge is derived from the framework of teteahedral alumina attracts cations are positively charged. The negative charge on NaA zeolite pores causing the occurrence of ion exchange. So in the few studies reported that the zeolite is able to reduce the levels of heavy

In a suspension, catalyst’s amount can affect the photocatalytic activity by blocking the light, dispersion/agglomeration of particles, adsorption-desorption of reactants and/ or intermediates, and charge carriers generation [44,45]. Regarding the graph, by building up the photocatalyst’s value from 20 to 50 and then to 100 mg a sharp decrease in concentration of the RB5 were observed. Afterwards, the dye degradation is decreased dramatically as a result of the building-up in the amount of the catalyst. The greatest percentage of degradation observed at 100 mg of catalyst regarded to optimal absorption of light and an appropriate number of active sites on the surface. Below the optimal amount, the number of catalytic active sites are less in-turn production of reactive species which results in lower oxidation efficiency. Above the optimal value of the photocatalyst, the observed lower activity could be results of an increase in the particle-particle interaction that consequences the increase in the turbidity of the solution. The opaque nature of the solution leads to inferior light absorption and fast charge recombination [46–48]. Finally, besides the fact that the role of the photocatalyst in adsorption of the reactant is vital, the light transmittance and blockage are extremely important,

5. The final result when all the dye emerges at the downstream side is shown in Figure 1.

Adsorption isotherms describe the equilibrium between the adsorbents and adsorbate to optimize the use of adsorbents and introduce a design and operation of adsorption systems by the correlation of experimental data through the theoretical equations. Isotherm studies were performed by mixing the optimum dose of both adsorbents with Pb2+ solution at different initial concentration (25-250 mg/l) and shaking for the optimum time at room temperature. The data was fitted into the following isotherms: Langmuir, Freundlich, Temkin and Dubinin-Raduskevich.