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 -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.
The Nernst equation can be used to calculate... A. cell potentials from standard cell potentials when the conditions of concentration and temperature are not standard B. standard cell potentials from standard reduction potentials C. cell potentials given only the temperature and reactant concentrations D. cell potentials from standard oxidation potentials E. the change in standard Gibbs free energy from standard cell potentials
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
18:53 please
In this aluminum concentration cell, the reaction would proceed spontaneously (from the left to the right compartment or right to left compartment)
Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to | the standard cell potentials on the last page of the note packet. Selected Answer: -54 A Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to the standard X cell potentials on the last page of the note packet. Selected Answer: 27.0
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
(iv) raised from 25 °C to 100 °C? Which of the following would result for any cell if the temperature was A. The cell potential would not change at all B. The cell potential would increase slightly C. The cell potential would decrease slightly D. It is impossible to determine. E. It would depend on the nature of the electrodes used.
Consider an electrochemical cell operating under standard conditions and at 25 °C. One half cell is the standard hydrogen electrode and the other contains dichromate ions and chromium(III) ions in an acidified solution. When the cell operates, the value of A G is O a. 770 x 105 J O b.257 x 105 J O C. 3.85 x 105J Od. 770 x 105J O e..257 x 105 J Of. 3.85 x 105 J O g. None of the above.