You were asked to record observations before, during and at the end of the experiment. Below are a list of possible observations that may apply to the electrolysis simulation. Read each observation very carefully and then select ALL observations which specifically apply to the electrolysis simulation. While the power supply was on, many small bubbles rose from the anode. Near the end of the experiment, small particles are observed floating in the solution around the anode. After the splint test, droplets are observed on the inside of the graduated cylinder. When a glowing wooden splint was applied to the collected gas in the graduated cylinder, a "pop" sound is heard and the splint ignites with a bright yellow flame. The colourless solution turned light blue. During the experiment, the measured current remained exactly the same. During the experiment, a gas was produced which displaced the 3M H2SO4 solution out of the graduated cylinder.

You were asked to record observations before, during and at the end of the experiment. Below are a list of possible observations that may apply to the electrolysis simulation. Read each observation very carefully and then select ALL observations which specifically apply to the electrolysis simulation. While the power supply was on, many small bubbles rose from the anode. Near the end of the experiment, small particles are observed floating in the solution around the anode. After the splint test, droplets are observed on the inside of the graduated cylinder. When a glowing wooden splint was applied to the collected gas in the graduated cylinder, a "pop" sound is heard and the splint ignites with a bright yellow flame. The colourless solution turned light blue. During the experiment, the measured current remained exactly the same. During the experiment, a gas was produced which displaced the 3M H2SO4 solution out of the graduated cylinder.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 76AP

See similar textbooks

Similar questions

the electroplating of a silver spoon, the spoon acts as thecathode and a piece of pure silver as the anode. Both dipinto a solution of silver cyanide (AgCN). Suppose that acurrent of 1.5 A is passed through such a cell for 22 minutesand that the spoon has a surface area of 16cm2. Calculatethe average thickness of the silver layer deposited onthe spoon, taking the density of silver to be 10.5gcm3.
A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie following data are collected: Corrosion Rate (mm/year) ph 0.03 13.00 0.06 12.00 0.16 11.00 0.22 10.00 0.25 9.00 0.25 8.00 0.25 7.00 0.25 6.00 0.25 5.00 0.27 4.00 0.37 3.00 0.38 2.80 0.63 2.80 1.00 2.80 Plot corrosion rate vs. pH. (HINT: Label the x axis with decreasing pH.) (a) How would you describe the dependence of corrosion on pH? (b) When the pH goes below 3, bubbles appear in the solution. What change takes place in the reduction half-reaction at low pH? (c) How do you explain the shape of the curve at the lowest pH? (Based on a graph in the Kirk-Otbmer Encyclopedia of Chemical Technology, 4th ed., vol 7. New York: John Wiley & Sons, p. 559.)
A current of 55,000 A is passed through a series of 100Hall–Héroult cells for 24 hours. Calculate the maximumtheoretical mass of aluminum that can be recovered.
. In the 1.0 M CuSO4 solution, the following species are present: Cu²+, SO42, H₂O, H3O+, and OH. Based on the observed changes that occurred in each electrode, write the RHR, OHR, and the balanced overall reaction of the electrolytic cell. The reactions should be consistent with the observations. For this part, refer to the following Setups: Electrodes Solution Current Time For the experimental data: Anode Carbon Setup 1 Observations at the anode Cathode Carbon 1.0 M CuSO4 1.50 A 20.00 minutes Initial mass of cathode (g) Initial appearance of cathode Final mass of cathode (g) Final appearance of cathode Setup 1 Table 8b-1. Data on the electrolysis of aqueous copper(II) sulfate. Parameter Initial mass of anode (g) Initial appearance of anode Final mass of anode (g) 14.02 Black-colored rod Black-colored rod Anode Carbon 14.03 Part of electrode that was submerged became a little darker; bubble formation was observed during electrolysis; electrolyte solution became acidic after…
You were asked to record observations betore, during and at the end of the experiment. Below are a list of possible observations that may apply to the electrolysis simulation. Read each observation very carefully and then select ALL observations which specifically apply to the electrolysis simulation. While the power supply was on, many small bubbles rose from the anode. Near the end of the experiment, small particles are observed floating in the solution around the anode. When a glowing wooden splint was applied to the collected gas in the graduate cylinder, a "pop" sound is heard and the splint ignites with a bright yellow flame After the splint test, droplets are observed on the inside of the graduated cylinder. The colourless solution turned light blue. During the experiment, the measured current remained exactly the same. During the experiment, a gas was produced which displaced the 3M H2SO4 solution out of the graduated.cydinder
Telephone Nu Email: tpchrdnova@gmail.com NAME: GRADE & SECTION: SUBJECT TEACHER: ACTIVITY SHEET in CHEMISTRY 2 WEEK 5-6 1. Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker contains a solution of MnO-4MnO4- in dilute sulfuric acid and has a Pt electrode. The other beaker contains a solution of Sn2+Sn2+ in dilute sulfuric acid, also with a Pt electrode. When the two electrodes are connected by a wire, current flows and a spontaneous reaction occurs that is described by the following balanced chemical equation: 2MnO-4(aq)+5Sn2+(aq)+16H+(aq)→2Mn2+(aq)+5Sn4+ (aq)+8H2O(1)2MnO4-(aq)+5 Sn2+(aq)+16H+(aq)→2Mn2+(aq)+5Sn4+(aq)+8H2O(1) For this galvanic cell, 1. write the half-reaction that occurs at each electrode. 2. indicate which electrode is the cathode and which is the anode. 3. indicate which electrode is positive and which is negative. ng, document you via e-mail cathe tht reflects fre allel to the in flecto ncor vith igl n
What is the difference between a calibration curve and a standard curve in analytical chemistry? How can you distinguish between a reversible and an irreversible electrochemical reaction? What is the difference between accuracy and precision in analytical chemistry?
Description The graph below shows how the mass of copper deposited during electrolysis varies with time. a Identify the dependent, independent and controlled variables. b State the relationship between the independent and dependent variables. c Calculate the rate (in gmin–1) of copper deposition (to two decimal places). d State two useful mathematical operations that could be performed on the graph. (Please don't give handwritten solution)
What are the advantages of glass electrode over hydrogen electrode? Please explain briefly.
Purification of chromium can be achieved by electrorefining chromium from an impure chromium anode onto a pure chromium cathode in an electrolytic cell. How many hours will it take to plate 10.5 kg of chromium onto the cathode if the current passed through the cell is held constant at 35.0 A? Assume the chromium in the electrolytic solution is present as Cr3+. time:_____ h
Find out the voltage supplied in an alkaline battery and what electrochemical reaction it uses. Suggest why the electrochemical reaction of alkaline battery is used in the remote control and wall clock.