may you please answer all three thank you!! Electrochemical Activity SeriesPrelab WorkGroup Members1. For the electrochemical cell below, label the cathode and the anode.Your Namewawalx [21= fowSartridgeY (aq)2. Given the data below, calculate the reduction potential for the metals.a. Metal 1: Ecell = 0.872 V, Eanode = -0.742 Vb. Metal 2: Ecell = 0.209 V, Eanode = -0.742 Vc. Metal 3: Ecell = 0.548 V, Eanode = -0.742 V3. Use the reduction potentials for the metals in question 2 to make an Activity Series. Organizethe Activity Series with the most reactive metal (best reducing agent) at the top and the leastreactive metal (worst reducing agent) at the bottom.

The objective is to label the electrodes in the cell diagram, compute the reduction potentials for…

Answered: 1. For the electrochemical cell below,…

1. For the electrochemical cell below, label the cathode and the anode. wever Love 2. Given the data below, calculate the reduction potential for the metals.

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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Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)
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A 1.250 g sample of bauxite (the primary ore of aluminum) was analyzed for aluminum. The sample was powderized and treated in concentrated nitric acid. The nitric acid was removed and solids were treated in hot water with added nitric acid. Insoluble solids were removed by gravity filtration. The solution was made basic by the slow addition of dilute ammonia forming the gelatinous precipitate (Al(OH), and Al,O,.x H2O). The precipitate was heated to coagulate it then filtered over filter paper. The paper and solids were placed in a porcelain crucible and the paper was ashed while the precipitate was ignited at 600°C to convert the precipitate to pure Al,O,. The mass of Al,O, recovered was 0.2890 g. The average mass of ash after charring 10 sheets of the identical filter paper was 0.0007 g. Calculate the percent aluminum in the bauxite ore sample.
1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the data
Note: This is an algorithm question so each attempt will have unique set of measurements. The following results were obtained when a sample of white cranberry juice was analyzed to determine its Vitamin C content. A 82.0 mL sample of the juice was placed in a flask with excess H2SO4, excess KI, and 11.00 mL of 0.07 000 M KIO3. Titration with thiosulfate solution required the use of 1.63 mL of 0.08826 M. Calculate the concentration of Vitamin C in the juice sample as mg Vit C per 100 mL juice. Here are some steps to help you work your way along the problem. All the reactions in the Background apply. • How many total millimoles of I are produced from the Reaction 4 between KI and KIO3? • How many millimoles of I are consumed in Reaction 3 with thiosulfate? . Using your previous two answers, how many millimoles of I reacted with the Vitamin C in the juice? • How many milligrams of Vitamin C were in the juice sample? • What is the concentration of Vitamin C in the juice sample expressed as…
(4b-102) Only using the list of ions below, form two ionic compounds that would be soluble in water, and two ionic compounds that would be insoluble in water. You should make four different compounds, but you may use ions more than once. Be sure to indicate which is which, and make sure your compounds are charge-balanced! Mg2+ Cu2+ k+ A13+ 02- PO43- CI OH For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).
Calculate the sum of coefficients for the following equation balanced for acidic conditions. 2+ XO7 + Y₂²+ → YO₂¹- + X²- Screen reader User: XO7 1 minus + Y₂ 2+ Answer: 25 × (149) YO₂ 1 minus + x2 minus
Volume vinegar used (mL)= 5.00 mL % from labe= l5 % Molarity of NaOH = 0.0976 M Titration volume measurements Trial 1 Trial 2 Trial 3 Inital volume NaOH (mL) 0.69 0.86 0.16 Final volume NaOH (mL) 43.47 43.36 43.03 Volume NaOH used (mL) Average volume NaOH used (mL) Average volume NaOH used (L) Moles NaOH used (from avg volume) Moles CH3COOH Molarity CH3COOH (mol/L) Mass CH3COOH (g) % (m/v) CH3COOH in vinegar
Illegal small-scale mining has been a major source of environmental pollution in Ghana. The quality of many water bodies has been affected by the acts of illegal small-scale mining. Use your knowledge in analytical process to systematically outline how you will go about to assess the extent of water pollution due to small-scale mining to make recommendations for those in authority.
A (aq) + ...B(aq) C(s) + D (aq) ... .. Experimental | Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 1.6 9.02 4 1.8 9.90 2.0 10.86 6. 2.2 10.90 7 2.4 10.88 8 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph.
-how to determine Kc/Kp from experimental data. -Fractional precipitation Provide examples for these 2
You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.