For the questions of Exp 20 Electrochemistry,Part A: Determination of the Faraday ConstantTable 1: Data collected from the electrolysisapparatus in part A of the experiment that is neededto determine the faraday constant.Time=3098 seccurrent (i) = 0.101 AVolume of H2 collected = 43.02 mLTemperature of water = 26.0 celsiusPressure = 760 mmHgAnswer the following questions with detailedcalculations.a) Determine the faraday constant (C/mol). For the questions of Exp 20 Electrochemistry,Part B: EMF of Galvanic CellTable 2: Electromotive force of the galvanic cell found throughthe mixtures of different solutions in part B of the experimentExperiment Solution A Electrode A Solution BElectrode B#4Sn2+SnC42+Cu#7Zn2+Zn0.1 M KCIAg WireAnswer the following question(s).a) Calculate E°cell for Experiment #4.

To determine the Faraday constant (C/mol) using the data from an electrolysis experiment, we'll…

Answered: For the questions of Exp 20…

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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Calculate the number of moles of electrons driven through an electrolytic cell with 3455 A of current passing through for 3.7 minutes. Round your answer to 2 decimal places.
Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.
I need help with the final question which is in bold. The previous questions and answers are needed to answer the final question In an electrolysis experiment similar to the one employed this experiment; a student observed that his unknown metal anode lost 0.238 grams while a total volume of 94.50 mL of hydrogen was being produced. The temperature of the solution was 25oC and the barometric pressure was 739 mm Hg. The difference between the water levels in the beaker and buret was negligible. The vapor pressure of water at 25oC is 23.8 mm Hg. Based on the information provided and the lab handout, what pressure of hydrogen is collected, in atmospheres? 9.41x10^-1 atm Using the data collected (in the previous problem), calculate the moles of hydrogen collected. 3.63x10^-3 mol Upon electrolysis, the metal is oxidized to a 2+ valence state. Based on this information, how many moles of metal are present? 3.63x10^-3 mol Use the mass of metal lost and moles from the previous problem to…
Calculate the number of moles of electrons driven through an electrolytic cell with 3304 A of current passing through for 3.5 minutes. Round your answer to 2 decimal places.
Calculate the number of moles of electrons driven through an electrolytic cell with 3676 A of current passing through for 4.4 minutes. Round your answer to 2 decimal places.
3q112 please answer with solutions thanks
Report all answers with the proper number of significant figures. In an electrolysis experiment similar to the one employed this experiment; a student observed that his unknown metal anode lost 0.238 grams while a total volume of 94.50 mL of hydrogen was being produced. The temperature of the solution was 25oC and the barometric pressure was 739 mm Hg. The difference between the water levels in the beaker and buret was negligible. The vapor pressure of water at 25oC is 23.8 mm Hg. Based on the information provided and the lab handout, what pressure of hydrogen is collected, in atmospheres? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:__________x10 units_____ Using the data collected, calculate the moles of hydrogen collected. Your Answer:__________x10 units_____ Upon electrolysis, the metal is oxidized to a 2+ valence state. Based on this information, how many moles of metal are present? Your Answer:__________x10 units_____ Use the…
Give typed explanation not a single word hand written otherwise leave it the answer is 0.03295 please help me understand how that is the answer
Suppose 830. mmol of electrons must be transported from one side of an electrochemical cell to another in 231. seconds. Calculate the size of electric current that must flow. Be sure your answer has the correct unit symbol and the correct number of significant digits.
Complete the following, providing written work for each part in order to receive credit: (a) Use shorthand notation to describe an electrochemical cell that contains gold (Au) and chromium (Cr) electrodes.(b) Determine which electrode will function as the anode and which will function as the cathode when the cell runs under standard conditions.(c) Calculate ΔG° for the cell under standard conditions. Enter your value for ΔG° in kJ below; do not actually enter the units.
Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)
Calculate the number of moles of electrons driven through an electrolytic cell with 3715 A of current passing through for 3.5 minutes. Round your answer to 2 decimal places.

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