Salt bridge A concentration cell similar to the one shown is composed of two Ni electrodes and solutions of different Ni²+ concentrations. The left compartment contains 0.482 M Ni²* , and the right compartment contains 1.48 M Ni²* . Calculate the cell potential for this reaction at 298 K. volts In this nickel concentration cell, the compartment on the left is the and the compartment on the right is the

Salt bridge A concentration cell similar to the one shown is composed of two Ni electrodes and solutions of different Ni²+ concentrations. The left compartment contains 0.482 M Ni²* , and the right compartment contains 1.48 M Ni²* . Calculate the cell potential for this reaction at 298 K. volts In this nickel concentration cell, the compartment on the left is the and the compartment on the right is the

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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Question

Salt bridge
A concentration cell similar to the one shown is composed of two Ni electrodes and solutions of different Ni?+ concentrations. The
left compartment contains 0.482 M Ni²+ , and the right compartment contains 1.48 M Ni²+ .
Calculate the cell potential for this reaction at 298 K.
volts
In this nickel concentration cell, the compartment on the left is the
v, and the compartment on the right is the

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A metal "X" is used as a "sacrificial" anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -0.89 V (minus 0.89 V). Your Answer:
1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -0.52 V (minus 0.52 V). 2.Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.46 volts.
Salt bridge A concentration cell similar to the one shown is composed of two Cr electrodes and solutions of different Cr3+ concentrations. The left compartment contains 1.14 M Cr3+ , and the right compartment contains 0.662 M Cr3+ . Calculate the cell potential for this reaction at 298 K. volts In this chromium concentration cell, the compartment on the left is the and the compartment on the right is the
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In this aluminum concentration cell, the reaction would proceed spontaneously (from the left to the right compartment or right to left compartment)
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the Relerences to access Important values Il needed lor this Salt bridge A concentration cell similar to the one shown is composed of two Al electrodes and solutions of different AIst concentrations. The left compartment contains 0.523 M AI+ , and the right compartment contains 0.380 M AI3+ . Calculate the cell potential for this reaction at 298 K. volts In this aluminum concentration cell, the reaction would proceed spontaneous v from the left to the right compartment from the right to the left compartment
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