阿拉 A concentration cell similar to the one shown is composed of two Mn electrodes and solutions of different Mn²+ concentrations. The left compartment contains 1.24 M Mn²+, and the right compartment contains 0.295 M Mn²+ Calculate the cell potential for this reaction at 298 K. volts In this manganese concentration cell, the compartment on the left is the the right is the and the compartment on

阿拉 A concentration cell similar to the one shown is composed of two Mn electrodes and solutions of different Mn²+ concentrations. The left compartment contains 1.24 M Mn²+, and the right compartment contains 0.295 M Mn²+ Calculate the cell potential for this reaction at 298 K. volts In this manganese concentration cell, the compartment on the left is the the right is the and the compartment on

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 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 -1.20 V (minus 1.20 V).
What are concentration cells? What is Ɛ in a concentration cell? What is the driving force for a concentration cell to produce a voltage? Is the higher or the lower ion concentration solution present at the anode? When the anode ion concentration is decreased and/or the cathode ion concentration is increased, both give rise to larger cell potentials. Why? Concentration cells are commonly used to calculate the value of equilibrium constants for various reactions. For example, the silver concentration cell can be used to determine the Ksp value for AgCl(s). To do so, NaCl is added to the anode compartment until no more precipitate forms. The Cl- in solution is then determined somehow. What happens to Ɛcellwhen NaCl is added to the anode compartment? To calculate the Ksp value, Ag+ must be calculated. Given the value of Ɛcell how is Ag+ determined at the anode?
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 -1.08 V (minus 1.08 V).
A cell consisting of a saturated calomel electrode and a lead ion electrode developed a potential of -0.5564 V when immersed in 25.00 mL of a sample. A 10.00 mL addition of standard 0.05000 M lead solution caused the potential to shift to -0.5090 V. Calculate the molar concentration of lead in the sample
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
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 -1.09 V (minus 1.09 V).
A copper-silver cell is set up. The copper ion concentration is 0.10 M. The concentration of silver ion is not known. The cell potential when measured was 0.422 V. Determine the concentration of silver ions in the cell.(GivenE0Ag+/Ag= +0.80 E0Cu2+/Cu = +0.34 V)
Salt bridge U A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of different Cu²+ concentrations. The left compartment contains 0.272 M Cu²+, and the right compartment contains 1.25 M Cu²+ . Calculate the cell potential for this reaction at 298 K. volts In this copper concentration cell, the compartment on the left is the + and the compartment on the right is the +
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
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 0.388 M Ni2+ , and the right compartment contains 1.32 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
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A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. V 'cell II