11- An electrolytic cell is set up using inert electrodes in an aqueous copper(II) sulfate solution. After an hour of electrolysis, the solution is tested. The concentration of copper(II) ions has decreased, while the concentration of hydrogen ions has increased. The mass of one electrode has also increased. Explain these observations using the half-reaction equation for each electrode.

11- An electrolytic cell is set up using inert electrodes in an aqueous copper(II) sulfate solution. After an hour of electrolysis, the solution is tested. The concentration of copper(II) ions has decreased, while the concentration of hydrogen ions has increased. The mass of one electrode has also increased. Explain these observations using the half-reaction equation for each electrode.

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...

See similar textbooks

Related questions

Q: Separate this redox reaction into its balanced component half-reactions. Use the symbol e for an…

A: The given redox reaction is

Q: Describe how you would design an experiment to determine the cell potential of a new, voltaic cell…

A: Answer - The cell potential, Ecell, is the measure of the potential difference between two half…

Q: What is the purpose of the salt bridge in a voltaic cell? O To increase solubility of the…

A: The purpose of the salt bridge in a voltaic cell has to be given.

Q: 1. In an electrolysis cell similar to the one employed in this experiment, a student observed that…

A: Given volume of hydrogen gas is 94.50 mL Given barometric pressure is 740mmHg and vapour pressure…

Q: Describe the anode and cathode of an electrolytic cell in which gold is to beplated on an object.

A: Electroplating produces a very thin coating of these expensive metals on the surfaces of cheaper…

Q: Three electrochemical cells were connected in series so that the same quantity of electrical current…

A: Given: First Cell: 1.15 g chromium metal was deposited from chromium (III) nitrate solution. Second…

Q: c. Identify the cathode and the anode and write their respective half-cell reactions. d. Write the…

A: Anode and cathode are two electrodes that are used in electrochemical reactions. An anode is the…

Q: 5. Define electrolytic cell and voltaic cell?

Q: Explain the similarities and differences between a voltaic and an electrolytic cell. Discuss how…

A: A galvanic cell or voltaic cell or electrochemical cell is the type of cell in which chemical energy…

Q: 16. In which direction do electrons flow in an electrochemical cell? a From the cathode to the anode…

A: Electrochemical cell converts chemical reaction into electrical energy. The cell consists of an…

Q: How many grams of cobalt may be formed by the passage of 3.71 amps for 2.68 hours through an…

A: According to the Faraday's first law of electrolysis, the amount of chemical change which will take…

Q: Upon completing a reaction in the lab, you determine the percent yield for the process to be 140%.…

Q: A 1.0 M solution of aluminum nitrate is placed in a beaker with a strip of aluminum metal. A 1.0 M…

Q: Which statement best explains the difference between an electrochemical cell and an electrolytic…

A: Electrochemical cell- This cell converts chemical energy to electrical energy.Electrolytic cell-…

Q: During an electrolysis experiment, the following species are present in solution: H+, CH3COOH,…

A: Oxidation is defined as process of addition of oxygen or an electronegative element to the…

Q: Which statement is not correct? O A voltaic cell is a type of electrochemical cell All…

A: Electrolysis is chemical decomposition of electrolyte in the aqueous state by the passage of…

Q: Separate this redox reaction into its balanced component half-reactions. Use the symbol e for an…

A: Given redox reaction is, Cl2 + 2 K ---> 2 KCl Note: In Redox reaction transfer of electrons…

Q: 39. Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the…

Q: In a Galvanic cell, the anode is labeled the negative cell and the cathode is labeled the positive…

A: we have to find -In a Galvanic cell, the anode is labelled as the negative cell and the cathode is…

Q: Predict which cation will be reduced first if the following mixture of molten salts undergoes…

A: The Cations in the given salts are, NaCl = Na+ CaCl2 = Ca2+ AgCl = Ag+

Q: What is an electrochemical reaction?

Question

100%

11- An electrolytic cell is set up using inert electrodes in an aqueous copper(II) sulfate solution.
After an hour of electrolysis, the solution is tested. The concentration of copper(II) ions has
decreased, while the concentration of hydrogen ions has increased. The mass of one electrode
has also increased. Explain these observations using the half-reaction equation for each
electrode.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

One of the differences between a voltaic cell and an electrolytic cell is that in an electrolytic cell, an electric current is produced by a chemical reaction electrons flow toward the anode a nonspontaneous reaction is forced to occur 02 gas is produced at the cathode oxidation occurs at the cathode
Explain chemically how an electrolytic cell works for both hydrolysis of water and electroplating.
3.What happens to the standard cell potential of a battery when temperature increases? A.The standard electrode potential will not be affected by any change in temperature. B.The standard electrode potential will always decrease when temperature increases. C.The standard electrode potential will always increase when temperature increases. D.The standard electrode potential may increase or decrease depending on the nature of the electrodes.
An unknown metal, X, has been deposited on the cathode of an electrolytic cell using an electric current of 3.30 Amps for a period of 25.0 mins: 2X2+ + 2 e– → X The mass of X collected at the cathode was 1.51 g. Identify the unknown metal, X.
Describe what is happening at the anode and cathode in a voltaic cell between copper (submerged in copper (II) sulfate) and iron (submerged in iron (II) sulfate). Reference Appendix L in the OpenStax textbook.
1. Complete the following table summarizing the general properties of the electrodes in an electrolytic cell. Electrode Oxidation or Reduction Sign of Electrode Anode Cathode
Over a period of time, the concentration of sulfuric acid in the lead storage battery of an automobile has decreased from 38.0 percent by mass (density = 1.29 g / mL) to 26.0 percent by mass (1.19 g/mL). Assume the volume of the acid remains constant at 734 mL. Calculate the total charge in coulombs supplied by the battery. How long (in hours) will it take to recharge the battery back to the original sulfuric acid using a current of 23.4 A?
Which of the following is a true statement regarding an electrolytic cell? Oxidation occurs at the cathode. Electrons flow from the cathode to the anode. All these statements are true. Electrical energy is used to cause a chemical reaction to occur that would be otherwise be nonspontaneous.
A chemist designs a galvanic cell that uses these two half-reactions:
2.What is the standard cell potential of an electrochemical cell? A.the sum of standard electrode potential of the two half-cells B.the standard electrode potential of the anode, relative to a hydrogen cell C.the difference between the standard electrode potential of the two half-cells D.the standard electrode potential of the cathode, relative to a hydrogen cell
When a rechargeable battery is recharged, it becomes a galvanic cell extra electrons are being stored in it the electrons used up by the battery are replaced it is like the function of an electrolytic cell
How is the amount of current flowing through an electrolytic cell related to the amount of product produced in the redox reaction? Match the items in the left column to the appropriate blanks in the sentences on the right. multiplied coulombs Avogadro's 1 mol Faraday's 1g ampers 6.022 x 10¹ mol volts divided The number of moles of electrons that have flowed in a given electrolysis cell can be determined by measuring the total charge that has flowed through the cell. If the amount of current flowing through the cell is by the time that the current flowed, the total charge that passed through the cell in that time can be found. The relationship between charge and the number of moles of electrons constant, which corresponds to the charge in is given by of of electrons. These relationships are used to solve problems involving the stoichiometry of electrolytic cells. Reset Help