Recent questions without a selected answer

0 votes

1 answer 78 views

Calculate the corrosion potential of a zinc-copper galvanic couple in which the zinc electrode has a concentration of 0.1 M and the copper electrode has a concentration of 0.01 M. The standard reduction potentials for Zn2+/Zn and Cu2+/Cu are -0.76 V and +0.34 V, respectively.

asked Jan 23 in ElectroChemistry by MAQShelton1 (1.7k points)

0 votes

1 answer 43 views

Calculate the corrosion potential of a silver metal in a solution containing 0.1 M silver nitrate and 1 M nitric acid given that the standard reduction potential of the Ag⁺/Ag couple is +0.80 V and the standard reduction potential of the NO₃⁻/NO₂⁻ couple is +0.96 V.

asked Jan 23 in ElectroChemistry by Latonya89F54 (2.2k points)

0 votes

1 answer 64 views

Calculate the corrosion potential of a pure copper metal electrode immersed in a 0.1 M solution of CuSO4 at 298 K, given that the standard electrode potential of Cu2+/Cu is +0.34 V and the standard potential of the hydrogen electrode is 0 V. Assume that activity coefficients for copper ions and sulfate ions are equal to 1.0 in the solution. What is the likelihood that this copper electrode will corrode in this given environment?

asked Jan 23 in ElectroChemistry by Maura45O7086 (2.5k points)

0 votes

1 answer 62 views

Calculate the corrosion potential of a nickel metal electrode in a 0.1 M NaCl solution with a pH of 7.2, given that the standard electrode potential for the Ni2+/Ni redox reaction is -0.25 V vs. the standard hydrogen electrode.

asked Jan 23 in ElectroChemistry by Annett65L392 (2.1k points)

0 votes

1 answer 62 views

Calculate the corrosion potential of a copper metal electrode in a solution containing 0.1M CuSO4 and 0.5M H2SO4 at 298K, given that the standard electrode potential of the Cu2+/Cu electrode is +0.34V and a hydrogen electrode is used as the reference electrode.

asked Jan 23 in ElectroChemistry by GreggTimperl (2.4k points)

0 votes

1 answer 57 views

Calculate the corrosion potential of a copper metal electrode in a 0.1 M CuSO4 solution at 25°C, given that the standard reduction potential of Cu2+/Cu is +0.34 V.

asked Jan 23 in ElectroChemistry by JackQ7308746 (2.0k points)

0 votes

1 answer 53 views

Calculate the corrosion potential of a copper electrode that is coupled with a silver electrode in a 0.010 M silver nitrate solution at 25°C. Given that the standard reduction potential for Ag+ + e- → Ag is +0.80V and for Cu2+ + 2e- → Cu is +0.34V. What is the potential of the copper electrode with respect to the standard hydrogen electrode?

asked Jan 23 in ElectroChemistry by SuzannaRayfo (1.8k points)

0 votes

1 answer 78 views

Calculate the corrosion potential of a copper electrode immersed in a 1 M CuSO4 solution in contact with a silver electrode immersed in a 1 M AgNO3 solution. Given that the standard reduction potentials of Cu2+/Cu and Ag+/Ag are +0.34 V and +0.80 V, respectively. Determine which electrode will corrode and which electrode will act as a cathode in the galvanic cell.

asked Jan 23 in ElectroChemistry by HoraceT7712 (2.0k points)

0 votes

1 answer 64 views

Calculate the corrosion potential of a copper electrode immersed in a 0.10 M solution of copper(II) sulfate at 25°C, given that the standard reduction potential of Cu2+/Cu is +0.34 V and the pH of the solution is 4.5.

asked Jan 23 in ElectroChemistry by JuliannSfd66 (2.0k points)

0 votes

1 answer 74 views

Calculate the corrosion potential for an iron electrode in a galvanic couple with a standard hydrogen electrode at 25°C if the concentration of Fe2+ ion is 0.05 M and pH is 7.

asked Jan 23 in ElectroChemistry by TerrieGaffne (1.6k points)

0 votes

1 answer 72 views

Calculate the corrosion potential for a pure iron (Fe) electrode in a 1 M HCl solution at 25°C, given that the standard reduction potential of Fe in acidic solution is -0.44 V.

asked Jan 23 in ElectroChemistry by AnibalX1615 (2.1k points)

0 votes

1 answer 57 views

Calculate the corrosion current density of an iron rod having a surface area of 15 cm², immersed in an acid solution (pH=3) with a temperature of 50°C. The concentration of iron ions (Fe²⁺) in the solution is 0.1 M, and the standard reduction potential of iron is -0.44 V. The Tafel slope obtained experimentally is 0.12 V/decade. Use the Tafel equation to calculate the corrosion current density (in A/cm²) of the iron rod.

asked Jan 23 in ElectroChemistry by ClaritaSifue (1.8k points)

0 votes

1 answer 65 views

Calculate the corrosion current density of a steel metal in contact with a copper metal, given that the corrosion potential of steel and copper are -0.58 V and +0.34 V, respectively. The temperature and pH of the solution are 25°C and 7, respectively. The surface area of the steel metal is 10 cm2 and the copper metal is a large area electrode.

asked Jan 23 in ElectroChemistry by DannieGuf001 (2.3k points)

0 votes

1 answer 73 views

Calculate the corrosion current density of a stainless steel electrode in a 0.5 M HCl solution at 25 degrees Celsius, given that the polarization resistance of the electrode is 200 ohms and the corrosion potential is -0.3 V vs. the standard hydrogen electrode (SHE).

asked Jan 23 in ElectroChemistry by RandolphWvo (1.9k points)

0 votes

1 answer 71 views

Calculate the corrosion current density of a metal M in a 0.5 M H2SO4 solution with a pH of 2.5, where the half-cell potential of the metal M is -0.8V and the standard hydrogen electrode potential is 0V. The temperature of the solution is 25°C and the density of the metal is 7.85 g/cm³.

asked Jan 23 in ElectroChemistry by PeteWirtz263 (2.1k points)

0 votes

1 answer 57 views

Calculate the corrosion current density of a copper metal in 1 M HCl solution at 25°C, given that the corrosion potential of copper electrode in the given environment is -0.35 V(SHE) and the exchange current density is 0.038 A/m². Also, determine the corrosion rate of copper in the same environment if the density of copper is 8.96 g/cm³.

asked Jan 23 in ElectroChemistry by Jerry12T3434 (1.7k points)

0 votes

1 answer 54 views

Calculate the corrosion current density for a zinc-copper galvanic couple, with a surface area of 10 cm² each, immersed in a 0.1 M copper sulfate solution and a 0.1 M zinc sulfate solution, respectively. Given that the exchange current density for the zinc and copper electrodes are 0.0035 A/cm² and 0.1184 A/cm², respectively, What will be the corrosion rate for the zinc electrode in micrometers per year?

asked Jan 23 in ElectroChemistry by SherrylP401 (2.4k points)

0 votes

1 answer 42 views

Calculate the corrosion current density for a steel pipe of diameter 10 cm and length 20 m, which is exposed to a 0.1 M HCl solution. The corrosion potential of steel in the given environment is -0.5 V (SHE), the Tafel slope is 0.12 V/decade, and the temperature is 25°C. Consider the density of steel to be 7.86 g/cm³ and the flow rate of the solution to be 5 L/min.

asked Jan 23 in ElectroChemistry by IsabellFrome (2.1k points)

0 votes

1 answer 66 views

Calculate the corrosion current density (in mA/cm²) of a silver electrode in a galvanic couple with a standard hydrogen electrode if the measured potential of the silver electrode is -0.25 V versus the standard hydrogen electrode at a temperature of 25 °C. The Tafel slope of the silver electrode is 30 mV/decade and the corrosion potential of silver in the given environment is -0.15 V.

asked Jan 23 in ElectroChemistry by AgustinSteed (2.2k points)

0 votes

1 answer 70 views

Calculate the corrosion current density (in mA/cm²) of a copper metal in a 3 M sulfuric acid solution at 25°C, given that the corrosion potential is -0.35 V and the Tafel constants are 120 mV/dec for the anodic reaction and 60 mV/dec for the cathodic reaction.

asked Jan 23 in ElectroChemistry by MarisolWebst (1.8k points)

Page:

« prev
1
...
692
693
694
695
696
697
698
699
700
...
1000
...
next »

Recent questions without a selected answer

Categories