Salt bridgeA concentration cell similar to the one shown is composed of two Al electrodes and solutions of different AP* concentrations. The left compartment contains 0.349 M AI*, and the right compartment contains 0.431 M A*Calculate the cel1 potential for this reaction at 298 K.voltsIn this aluminum concentration cell, the reaction would proceed spontaneously

Left compartment : anode = oxidation Right compartment : cathode = reduction Anode : Al .....>…

Answered: Salt bridge A concentration cell…

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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A certain half-reaction has a standard reduction potential E 0.57 V. An engineer proposes using this half-reaction at the anode of a galvanic red cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction E red - Ov potential that the half-reaction used at yes, there is a minimum. the cathode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Is there a maximum standard reduction potential that the half-reaction used at yes, there is a maximum. E red the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper no maximum limit, check the "no" box.
Electrolysis can be used to purify silver. What mass of silver would plate onto the pure electrode if a current of 6.8 A flowed through the cell for 72 minutes?
Salt bridge A concentration cell similar to the one shown is composed of two Mn electrodes and solutions of different Mn+ concentrations. The left compartment contains 1.02 M Mn2*, and the right compartment contains 0.835 M Mn*. Calculate the cell potential for this reaction at 298 K. volts In this manganese concentration cell, the compartment on the left is the and the compartment on the right is the
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Determine the number of moles of electrons being exchanged in the resulting redox reaction. Select one: a. 1 mol of electrons b. 4 mol of electrons c. 5 mol of electrons d. 2 mol of electrons e. 3 mol of electrons
Using a table of standard reductions potentials calculate the solubility product (Ksp) of the compound assigned to you. Write down the two balanced half-reactions and their voltages. Label the anode, the cathode, which cell is the oxidation and reduction and whether it is positive or negative. Indicate the direction of electron flow, the concentrations of all ionic species and the composition of the electrodes. Calculate the voltage of the cell and then, using the voltage, calculate the Ksp of your compound. MUST SHOW ALL WORK! Calculation of the Ksp of Ag2CO3 Half reactions: Overall Voltage:
. At 25 C, the standard hydrogen electrode (SHE) has a half-cell potential that is defined to be 0.00 volts. If the pH is increased at this electrode (keeping everything else the same), at what pH will the half-cell potential be equal to -0.521 volts?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell AG K E A 77. kJ/mol -14 3.24 x 10 0.80 V 119. kJ/mol 20 7.05 x 10 -1.23 V 60. kJ/mol -11 3.08 x 10 -0.62 V
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. experimental standard cell potential, Eocell, for the reaction=1.06 experimental standard state free energy change, ΔGo, for the reaction =2.69e35 Calculate the experimental equilibrium constant, K, for the reaction Your answer should have 3 sig figs
The half reaction for the formation of magnesium metal upon electrolysis of molten MgCl2 is Mg2+ + 2e- --> Mg. How much current should pass through the molten solution for 4.00 x 103 seconds to produce 30.2 g Mg?
A certain half-reaction has a standard reduction potential Ed+0.57 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. red Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper Smit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at…
In this aluminum concentration cell, the reaction would proceed spontaneously (from the left to the right compartment or right to left compartment)
calculated quantities (Check the box next to any that are wrong.) 0 K 0 E cell n AG 44 A 2 -255. kJ/mol 4.72 x 10 О -1.32 V -31 B 2 - 176. kJ/mol 1.47 x 10 ○ -0.91 V 44 C 2 255. kJ/mol 4.72 x 10 -1.32 V ☑

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