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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 AgustinSteed (2.2k points)

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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)

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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 DemetriusCha (1.7k points)

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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 MarciaBrooke (1.8k 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 KyleSchlemme (2.1k points)

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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 AundreaWhitf (1.8k points)

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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 WilburnMcCor (1.8k 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 CharleneLemu (1.7k points)

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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 MOIRoderick9 (1.8k points)

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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 TinaKesler6 (1.9k 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 JoelPrentice (1.4k points)

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Calculate the change in entropy for the combustion of methane gas (CH4) at constant pressure and temperature of 298 K. The products of the reaction are carbon dioxide gas (CO2) and water vapor (H2O). The molar entropy of CH4, CO2 and H2O at 298 K are 186.3 J/K/mol, 213.7 J/K/mol, and 188.8 J/K/mol, respectively.

asked Jan 23 in Chemical thermodynamics by TaylaBromby8 (2.2k points)

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Calculate the change in entropy and enthalpy for the reaction of iron (III) oxide with carbon monoxide to form iron and carbon dioxide, given the following information:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)ΔH°f (Fe2O3) = -824.2 kJ/molΔH°f (CO) = -110.5 kJ/molΔH°f (Fe) = 0 kJ/molΔH°f (CO2) = -393.5 kJ/molΔS° (Fe2O3) = 87.4 J/K molΔS° (CO) = 197.9 J/K molΔS° (Fe) = 27.3 J/K molΔS° (CO2) = 213.6 J/K mol

asked Jan 23 in Inorganic Chemistry by ShadArchie3 (1.7k points)

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Calculate the change in entropy (ΔS) of the following reaction at 298 K:2SO2(g) + O2(g) → 2SO3(g) Given the standard molar entropies at 298 K: ΔS°(SO2,g) = 248.2 J/Kmol ΔS°(O2,g) = 205.0 J/Kmol ΔS°(SO3,g) = 256.2 J/Kmol

asked Jan 23 in Chemical thermodynamics by ChuWegener2 (2.1k points)

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Calculate the change in entropy (ΔS) for the reaction in which 3 moles of carbon monoxide (CO) gas is burned with excess oxygen gas to form 3 moles of carbon dioxide (CO2) gas. The reaction is carried out at constant pressure and a temperature of 298 K.

asked Jan 23 in Inorganic Chemistry by QJXClarice2 (2.5k points)

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Calculate the change in entropy (in J/K) for the following reaction at 298 K: 2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l) Given the following standard entropy values (in J/K): CH3OH (l): 126.6, O2 (g): 205.0, CO2 (g): 213.6, H2O (l): 69.9

asked Jan 23 in Chemical thermodynamics by RondaSkeyhil (1.7k points)

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Calculate the change in enthalpy for the reaction CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) given that the enthalpies of formation for CH4 (g), CO2 (g) and H2O (l) are -74.81 kJ/mol, -393.51 kJ/mol and -285.83 kJ/mol respectively.

asked Jan 23 in Physical Chemistry by CorneliusBur (2.1k points)

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Calculate the change in enthalpy for the following chemical reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given that the enthalpies of formation for CH4(g), CO2(g), and H2O(l) are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol respectively.

asked Jan 23 in Chemical reactions by ZKLBarbra368 (2.3k points)

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Calculate the change in enthalpy for the combustion of 2 moles of methane gas (CH4) at a constant pressure of 1 atmosphere and a temperature of 298 K. Given the standard enthalpy of formation for methane is -74.81 kJ/mol.

asked Jan 23 in Physical Chemistry by JadaMeece33 (1.6k points)

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Calculate the change in enthalpy and entropy for the reaction Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) at 25°C given the following data:- ΔH°f for MgCl2(aq) = -641.3 kJ/mol- ΔS°f for MgCl2(aq) = -200.9 J/K/mol- ΔH°f for H2(g) = 0 kJ/mol- ΔS°f for H2(g) = 130.7 J/K/mol- ΔH°f for HCl(aq) = -167 kJ/mol- ΔS°f for HCl(aq) = -18.8 J/K/mol- ΔH°f for Mg(s) = 0 kJ/mol- ΔS°f for Mg(s) = 32.7 J/K/molAssume that ΔH°f and ΔS°f are independent of temperature.

asked Jan 23 in Inorganic Chemistry by ArleneLeichh (2.1k points)

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