4- Create a diagram (step-by-step flowchart) of the procedure for the "Color Absorption by a Cobalt(II) ChlorideSolution". Your diagram should be clear and easy to follow by anybody who will perform the experiment.5- Rearrange the equation below to solve for n;. You MUST show the step by step work (without thisrequirement the question will be considered as no answered)AE = hv=-2.18 × 10-18 J(--nj nj6- On the energy diagram, draw an arrow to show the absorption from n = 1 to n = 5 and the emission from n =4 to n = 2. Use different color pens (pencils) and label each transition.7- Explain the physical significance of a negative value for AE. Why must Ephoton always be positive, whileAE can be positive or negative?8- Rearrange the equation to solve for lambda. E = hc. You MUST show the step by step work (without thisrequirement the question will be considered as no answered)

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4- Create a diagram (step-by-step flowchart) of the procedure for the "Color Absorption by a Cobalt(II) Chloride Solution". Your diagram should be clear and easy to follow by anybody who will perform the experiment.

4- Create a diagram (step-by-step flowchart) of the procedure for the "Color Absorption by a Cobalt(II) Chloride Solution". Your diagram should be clear and easy to follow by anybody who will perform the experiment.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…
3. The pH of blood is buffered by a mixture of HCO3- (bicarbonate) and H2CO3 (carbonic acid).i. Write out an equation that shows a reaction of H+ with HCO3-iii. Recall that H2CO3 (aq) decomposes readily. Write a chemical equation to describe this decomposition. The pH of blood is buffered by a mixture of HCO3- (bicarbonate) and H2CO3 (carbonic acid). Write out an equation that shows a reaction of H+ with HCO-3. Recall that H2CO3 (aq) decomposes readily. Write a chemical equation to describe this decomposition. Consider your response to the last question and explain how bicarbonate and carbonic acid are generated by the dissolving of CO2 in water (Hint: The reaction for “ii” is reversible.)
I completed my pre-lab and want it reviewed for corrections
In Part 1 of the experiment, you will generate a calibration curve in order to determine el for this reaction. In order to ensure that the [Fe(SCN)2*] for these calibration solutions is accurately known, a large excess of SCN is used, so that the equilibrium for these solutions lies heavily to the products, and we can assume all of the Fe2* added becomes Fe(SCN)2*. In Part 2, you will observe solutions prepared with various initial reactant concentrations in order to determine Keg for the formation of iron(II) thiocyanate.
Experiment 3: The Equilibrium State Introduction In this experiment, you will quantitatively assess the equilibrium constant for the reaction of the iron (III) cation complexing with a thiocyanate anion (SCN–) to form the red iron (III) thiocyanate complex, Fe(SCN)2+. (1) If Kc is a large number (>1), then the chemical equilibrium favors the formation of product (large numerator). If Kc is a small number (<1), then the chemical equilibrium favors the formation of reactants (large denominator). In this simulated experiment, several solutions of varying initial concentrations of reactants (and product) are to be evaluated. Despite the different concentrations, the equilibrium constants calculated from their equilibrium concentrations should be the same, as long as the temperature is kept constant.