Recent questions in Chemistry

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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 DannyFlowers (870 points)

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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 ClariceScott (590 points)

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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 AnnelieseSum (470 points)

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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 NumbersJacks (870 points)

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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 GrettaCopley (450 points)

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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 JeffereyHail (430 points)

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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 CurtMinnis56 (570 points)

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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 KirbyDent557 (530 points)

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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 GarlandSouku (510 points)

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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 MadisonJ035 (470 points)

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1 answer 54 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 MargieSmorgo (600 points)

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Calculate the concentration of Cu2+ ions in a 0.1 M CuSO4 solution using the given standard reduction potential of Cu2+/Cu electrode and the measured cell potential. The electrode potential of the cell is 0.78 V and temperature is 25°C.

asked Jan 23 in ElectroChemistry by ELGVirgie318 (370 points)

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1 answer 53 views

Calculate the concentration of Cl^- ions in a solution if the electrode potential of a Pt/AgCl electrode in the solution is measured to be +0.222 V versus the standard hydrogen electrode (SHE) at 25°C. The standard electrode potential for the reaction AgCl(s) + e^- → Ag(s) + Cl^- is +0.222 V versus SHE at 25°C. Assume the activity coefficient of Cl^- ions in the solution is equal to 1.

asked Jan 23 in ElectroChemistry by JoleenGoethe (610 points)

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Calculate the change in internal energy of a system that releases 350 J of heat to the surroundings and does 200 J of work on its surroundings?

asked Jan 23 in Physical Chemistry by RaquelGendro (430 points)

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1 answer 36 views

Calculate the change in Gibbs free energy for the reaction between hydrogen gas and iodine gas that forms hydrogen iodide gas. The balanced equation is as follows:H2(g) + I2(g) → 2HI(g)Assume a temperature of 298 K and use the following standard molar free energy of formation values:∆Gf° (HI) = -17.4 kJ/mol∆Gf° (H2) = 0 kJ/mol∆Gf° (I2) = 0 kJ/mol

asked Jan 23 in Chemical thermodynamics by KevinBrazeno (350 points)

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1 answer 50 views

Calculate the change in Gibbs free energy for the electrochemical reaction, given the standard reduction potentials of the reactants and products:Cu2+ (aq) + 2e- → Cu (s)E° = +0.34 VFe2+ (aq) + 2e- → Fe (s)E° = -0.44 V

asked Jan 23 in ElectroChemistry by WiltonRuatok (430 points)

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Calculate the change in entropy when 1 mole of methane gas (CH4) is burned completely in oxygen gas (O2) at constant pressure and 298 K.

asked Jan 23 in Chemical thermodynamics by MandyFinley (690 points)

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1 answer 52 views

Calculate the change in entropy when 1 mole of an ideal gas is compressed from 4 L to 1 L irreversibly at a temperature of 298 K.

asked Jan 23 in Physical Chemistry by CarrieGabel2 (510 points)

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1 answer 39 views

Calculate the change in entropy of the system when 2 moles of ammonia react to form 3 moles of hydrogen gas and 1 mole of nitrogen gas. The reaction takes place at a constant temperature of 298 K and at a pressure of 1 atm. The molar entropy of each component in the reaction is given below:Ammonia: 192.5 J/K·molHydrogen gas: 130.6 J/K·molNitrogen gas: 191.6 J/K·mol

asked Jan 23 in Chemical thermodynamics by AlisonEastwo (660 points)

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Calculate the change in entropy for the reaction: 2H2(g) + O2(g) → 2H2O(g)if the standard entropy values of H2, O2, and H2O are 130.7 J/mol*K, 205.0 J/mol*K, and 188.7 J/mol*K, respectively.

asked Jan 23 in Inorganic Chemistry by RolandoT7187 (370 points)

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