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Calculate the standard cell potential of the following electrochemical cell at 298 K, given the half-reactions and their standard reduction potentials in brackets:Cu(s) | Cu^2+(0.001 M) || Ag+(0.1 M) | Ag(s)

asked 4 days ago in Physical Chemistry by VirgilioGree (470 points)

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Calculate the standard enthalpy of formation (ΔH°f) of carbon dioxide (CO2) at 25°C given the following data:CO(g) + 1/2 O2(g) → CO2(g) ΔH° = -283.3 kJ/molC(s) + O2(g) → CO2(g) ΔH° = -393.5 kJ/molΔH°f (C(s)) = 0 kJ/molΔH°f (O2(g)) = 0 kJ/mol

asked 4 days ago in ThermoChemistry by MichaelBolin (370 points)

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Calculate the polarization resistance of a copper electrode in a 0.1 M copper sulfate solution at 25°C, given that the current density is 10 mA/cm² and the exchange current density is 0.1 mA/cm². The Tafel slope is 30 mV/decade.

asked 5 days ago in ElectroChemistry by MauricioMaj (630 points)

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Calculate the standard enthalpy change for the reaction where 50 ml of 0.1 M hydrochloric acid reacts with 50 ml of 0.1 M sodium hydroxide solution. The temperature change observed during the reaction was 5°C and the specific heat capacity of the solution is 4.18 J/g°C.

asked 4 days ago in Chemical thermodynamics by CandaceGarra (610 points)

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Calculate the standard enthalpy change for the formation of ammonium chloride (NH4Cl) from its constituent elements, nitrogen (N2), hydrogen (H2), and chlorine (Cl2), given the following information:Reaction equation: N2(g) + 4H2(g) + 2Cl2(g) → 2NH4Cl(s)Standard enthalpy of formation for NH4Cl: -314.4 kJ/molStandard enthalpy of formation for N2(g): 0 kJ/molStandard enthalpy of formation for H2(g): 0 kJ/molStandard enthalpy of formation for Cl2(g): 0 kJ/mol Express your answer in kilojoules per mole (kJ/mol).

asked 4 days ago in Chemical thermodynamics by NikiCoombs07 (590 points)

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Calculate the polarization of a copper electrode immersed in a 0.1 M CuSO4 solution at 25°C when it is coupled to a hydrogen electrode with a hydrogen pressure of 1 atm. Given that the standard reduction potential of Cu2+|Cu electrode is 0.34 V and the standard reduction potential of H+|H2 electrode is 0 V at 25°C.

asked 5 days ago in ElectroChemistry by EldonHyman82 (490 points)

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Calculate the standard free energy change (ΔG°) for the following redox reaction: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)Given: ΔG°f (Zn2+) = -153.9 kJ/mol ΔG°f (H+) = 0 kJ/mol ΔG°f (H2) = 0 kJ/mol ΔG°f (Zn) = 0 kJ/mol

asked 4 days ago in Chemical thermodynamics by DemetriaOhma (350 points)

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Calculate the standard electrode potential of the following reaction: Cu2+(aq) + 2e- ⇌ Cu(s) Given that the standard reduction potential of Cu2+(aq) is +0.34 V and the standard electrode potential of hydrogen electrode is 0.00 V.

asked 4 days ago in Chemical thermodynamics by MohammadC566 (390 points)

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Calculate the standard enthalpy change for the following reaction, given the standard enthalpies of formation:2Fe (s) + 3Cl2 (g) → 2FeCl3 (s)ΔH°f(FeCl3) = -399.4 kJ/molΔH°f(Fe) = 0 kJ/molΔH°f(Cl2) = 0 kJ/mol

asked 4 days ago in Chemical thermodynamics by MackBeckham (450 points)

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1 answer 24 views

Consider the following chemical equation: 2 SO2(g) + O2(g) ⇌ 2 SO3(g)At equilibrium, the concentration of SO2 was found to be 0.10 M, the concentration of O2 was found to be 0.20 M, and the concentration of SO3 was found to be 0.30 M. What is the value of the equilibrium constant (Kc) for this reaction at the given temperature?

asked 4 days ago in Chemical equilibrium by MeredithBren (290 points)

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Calculate the standard enthalpy change for the reaction of 2 moles of liquid ethanol with 3 moles of gaseous oxygen to form 2 moles of liquid acetic acid and 3 moles of gaseous water at 1 atm and 25°C, given the standard enthalpy of formation of ethanol, acetic acid, and water are -277.6 kJ/mol, -487.5 kJ/mol, and -285.8 kJ/mol respectively.

asked 4 days ago in Chemical thermodynamics by LatashaKerse (390 points)

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Describe the steps involved in the preparation of 2,4-dichlorobenzoic acid from benzoic acid and chlorine gas, including the chemical reactions that occur during the process, the reagents required, the conditions required for each step, and the yields of each intermediate and final product.

asked 4 days ago in Chemical synthesis by Raphael64O24 (690 points)

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Calculate the standard enthalpy change for the vaporization of water at its normal boiling point of 100 degrees Celsius and a pressure of 1 atm. The molar enthalpy of vaporization for water is 40.7 kJ/mol. What is the amount of heat required to vaporize 100 g of water?

asked 4 days ago in Chemical thermodynamics by ChassidyMcCo (490 points)

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1 answer 24 views

Consider an electrochemical cell consisting of a zinc electrode in one half-cell and a copper electrode in the other half-cell. The zinc electrode has a surface area of 5 cm² and is placed in a 0.1 M ZnSO₄ solution, while the copper electrode has a surface area of 10 cm² and is placed in a 1.0 M CuSO₄ solution. Calculate the polarization of the cell when a current of 0.5 A is passed through it.

asked 4 days ago in ElectroChemistry by JamesCutler4 (250 points)

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1 answer 28 views

Calculate the standard enthalpy change for the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O), given the following information:- Heat capacity of the solution = 4.18 J/g°C- Volume of the solution = 50 mL- Concentration of HCl = 0.25 M- Concentration of NaOH = 0.10 M

asked 4 days ago in Chemical thermodynamics by BennettThorn (530 points)

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1 answer 30 views

Calculate the standard enthalpy change for the complete combustion of methane (CH4) at constant pressure and 298 K, given that the standard enthalpies of formation for CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively.

asked 4 days ago in Chemical thermodynamics by ArcherPcc770 (550 points)

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1 answer 35 views

Calculate the reaction quotient, Qc, for the reaction: 2 NO2 (g) + Cl2 (g) ⇌ 2 NO2Cl (g)At a certain temperature, the concentrations were found to be: [NO2] = 0.15 M, [Cl2] = 0.20 M, and [NO2Cl] = 0.10 M.Is the reaction at equilibrium? If not, which direction would the reaction proceed to reach equilibrium?

asked 5 days ago in Chemical thermodynamics by GQABrian353 (650 points)

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Calculate the number of electrons transferred when 1 mole of magnesium is oxidized to form magnesium ions in an electrochemical cell. The balanced half-reaction is Mg → Mg2+ + 2e-.

asked 5 days ago in ElectroChemistry by KristyDobos (430 points)

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Calculate the standard enthalpy change for the reaction between 50 mL of 1.0 M HCl and 50 mL of 1.0 M NaOH at 25°C given that the temperature of the resultant solution is 31.2°C and the specific heat capacity of the solution is 4.184 J/g°C.

asked 4 days ago in Chemical thermodynamics by DanielleBouc (490 points)

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1 answer 33 views

Calculate the standard electrode potential for the following reaction: Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)Given: Standard reduction potential for Ag+ + e- → Ag is 0.80 VStandard reduction potential for Cu2+ + 2e- → Cu is 0.34 V

asked 4 days ago in ElectroChemistry by Melinda41J1 (490 points)

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