. Iron metal corrodes when exposed to a moist atmosphere. The methods we have to protect iron structures from corrosion are: painting it, affixing a sacrificial metal or applying a low current. A suitable sacrificial metal is O nickel O magnesium O gold O copper Next

. Iron metal corrodes when exposed to a moist atmosphere. The methods we have to protect iron structures from corrosion are: painting it, affixing a sacrificial metal or applying a low current. A suitable sacrificial metal is O nickel O magnesium O gold O copper Next

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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If you constructed a cell with a copper electrode in contact with a 0.1 M solution of Cu2+ ions in onecell compartment and a copper electrode in contact with a 0.001 M solution in the othercompartment would a cell potential develop or would the potential of the cell be 0.00 V? (HINT:What would the Nernst equation for this cell look like?) Feel free to construct this cell and measureits potential if you wish to check your answer.
Which metal.would be suitable for use as a sacrificial anode for iron? OAu O Sn OMg OPt
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:
The decomposition of NaCl(l) into Na(l) and Cl2(g) is thermodynamically unfavorable. The decomposition requires the input of energy from an external source. The diagram represents an electrolytic cell that can be used to drive the decomposition reaction. Which of the following identifies a flaw in the representation? Oxidation is occurring at the anode. A Molten N a is shown at the cathode. B An external source of energy is not shown. C The direction of the electron flow in the wires is incorrect. D
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.
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).
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).
deposit 3.60 g of tin to achieve an adequate coating. If your electrolysis cell (using Sn) runs at - Sn(s)] 2. Suppose that you need a coating of rhodium (a precious metal) on a part that is to be used as a
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).
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2. Tell whether each of these statements are true and false. If false, rewite it to make it a correct statement. Oxidation always occurs at the anode of an electrochemical cell. The anode of a voltaic cell is the ite of reduction and is negative. Standard conditions for electrochemical cells are a concentration of 1.0 M for disolved species and a pressure of 1 bar for gases. The potential of a voltaic cell does not change with temperature. All product-favored oxidation-reduction reactions have a standard cell voltage E°cell, with a negative sign.
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.500 M and the concentration of the ion at the cathode is 1.50 M. Use the standard reduction potentials from Appendix L in our textbook.