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Consider an electrochemical cell containing a copper electrode in a 0.5 M CuSO4 solution and a silver electrode in a 1.0 M AgNO3 solution. Calculate the current density at a temperature of 25°C given that the copper electrode has a surface area of 5 cm² and the silver electrode has a surface area of 10 cm². The standard reduction potentials for Cu²⁺ and Ag⁺ are -0.34 V and 0.80 V, respectively. Use the Nernst equation to calculate the cell potential and then use Ohm's law to calculate the current density.

asked Feb 3 in ElectroChemistry by SimaSimone3 (510 points)

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Calculate the standard enthalpy of formation of propane (C3H8) given the following data:- Standard enthalpy of formation of CO2(g) = -393.5 kJ/mol- Standard enthalpy of formation of H2O(l) = -285.8 kJ/mol- Standard enthalpy of combustion of propane at constant pressure = -2220.1 kJ/mol

asked Feb 3 in Chemical thermodynamics by ShannaFord50 (460 points)

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Consider a solution of gas X in contact with a solid surface at a constant temperature. The Langmuir adsorption isotherm for this system is represented by the equation /= _/(1+), where is the partial pressure of gas X, is the volume of the gas, _ is the saturation pressure of the gas, and is the Langmuir adsorption constant. Suppose a student conducts an experiment to investigate the Langmuir adsorption isotherm for gas X on a particular solid surface. They measure the partial pressure of the gas at various volumes and obtain the following results: (mL/g) : 2.0 2.5 3.0 3.5 4.0 (atm) : 0.2 0.4 0.6 0.8 1.0 Using these values, what is the Langmuir adsorption constant, , for the given system?

asked Feb 3 in Surface Chemistry by AldaBartos98 (230 points)

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Calculate the standard enthalpy change (in kJ/mol) for the following chemical reaction at 298 K:2SO2(g) + O2(g) → 2SO3(g)Given the standard enthalpies of formation (∆Hf°) at 298 K for SO2(g), O2(g), and SO3(g) are -296.8 kJ/mol, 0 kJ/mol, and -396.0 kJ/mol, respectively.

asked Feb 3 in Physical Chemistry by TajPeyton117 (450 points)

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Calculate the number of electrons transferred during the following redox reaction: Cu(s) + 2Ag+ --> Cu2+ + 2Ag(s)

asked Feb 3 in ElectroChemistry by SelenaBarrag (410 points)

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Calculate the reaction quotient (Qc) for the following reaction at 298 K and 1 atm: 2 NO2(g) + F2(g) ⇌ 2 NO2F(g)Given the molar concentrations of reactants and products are [NO2] = 0.25 M, [F2] = 0.15 M, and [NO2F] = 0.10 M at equilibrium.

asked Feb 3 in Chemical thermodynamics by MabelCoulter (270 points)

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Calculate the standard enthalpy change for the reaction below, given the standard enthalpy of formation values: 2CO(g) + O2(g) → 2CO2(g)ΔH°f (CO) = -110.5 kJ/molΔH°f (O2) = 0 kJ/molΔH°f (CO2) = -393.5 kJ/mol

asked Feb 3 in Chemical thermodynamics by JuanHayman80 (590 points)

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Consider a cell consisting of a zinc electrode in 1.0 M ZnSO4 solution and a copper electrode in 1.0 M CuSO4 solution. Calculate the standard cell potential of the cell at 25°C, given that the standard electrode potential for the zinc electrode is -0.76 V and for the copper electrode is +0.34 V.

asked Feb 3 in ElectroChemistry by ErnestinaB30 (270 points)

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Calculate the standard Gibbs free energy change ($\Delta G^{\circ}$) for the following reaction at 298 K:2Fe(s) + 3/2O2(g) → Fe2O3(s) Given: Standard enthalpy of formation of Fe2O3(s) = -822.2 kJ/molStandard enthalpy of formation of Fe(s) = 0 kJ/molStandard entropy change for the reaction = +87.4 J/mol K

asked Feb 3 in Chemical thermodynamics by CecilB463053 (330 points)

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Certainly! Here's a precise problem for the student to solve:Calculate the standard enthalpy change ($\Delta H^\circ$) for the dissolution reaction of 5.00 g of lithium chloride ($\text{LiCl}$) in 150.0 mL of water, given that the density of water is 1.00 g/mL and the final temperature of the solution is 25.0$^\circ$C. The molar enthalpy of solution of $\text{LiCl}$ is -3.00 kJ/mol.

asked Feb 3 in Chemical thermodynamics by GwendolynLin (290 points)

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Calculate the standard free energy change, ΔG°, for the following redox reaction:2Fe2+ (aq) + H2O2 (aq) → 2Fe3+ (aq) + 2OH- (aq)Given the following half-reactions and their respective standard reduction potentials:Fe3+ (aq) + e- -> Fe2+ (aq) E° = +0.77 VH2O2 (aq) + 2H+ (aq) + 2e- ⟶ 2H2O (l) E° = +1.78 V

asked Feb 3 in Chemical thermodynamics by MillieFowlke (550 points)

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1 answer 42 views

Calculate the standard enthalpy change (∆H°) for the precipitation reaction between aqueous solutions of lead(II) nitrate [Pb(NO3)2] and potassium iodide (KI) producing solid lead(II) iodide (PbI2) and aqueous potassium nitrate (KNO3) at a temperature of 25°C.

asked Feb 3 in Chemical thermodynamics by WindyBirdwoo (390 points)

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1 answer 39 views

Calculate the standard enthalpy change for the formation of methane gas (CH4) from its elements carbon (solid, graphite) and hydrogen gas (H2) given the following data:ΔHf° (C(graphite)) = 0 kJ/molΔHf° (H2(g)) = 0 kJ/molΔHc° (CH4(g)) = -890.4 kJ/mol

asked Feb 3 in Chemical thermodynamics by SKTFern80161 (350 points)

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Calculate the standard enthalpy change (∆H°) for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) given the following information:- Balanced chemical equation: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)- ∆H°f of NaCl(aq) = -407.3 kJ/mol- ∆H°f of H2O(l) = -285.8 kJ/mol- Heat capacity of the system, Cp = 4.18 J/g.K- Mass of the HCl solution used = 50.0 g- Concentration of HCl solution = 0.100 M- Volume of NaOH solution used = 100.0 mL- Concentration of NaOH solution = 0.200 MAssume that the specific heat of the solution is equal to that of water at 4.18 J/g.K and that the density o

asked Feb 3 in Chemical thermodynamics by FayeJle84610 (330 points)

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1 answer 43 views

Calculate the specific surface area of a catalyst using BET theory, given that the quantity of gas physically adsorbed at a certain temperature and pressure is 0.25 moles, the molar volume of the gas is 22.4 L/mol, the weight of the catalyst used is 0.5 g, and the monolayer coverage of the adsorbate is 0.2.

asked Feb 3 in Surface Chemistry by CathyCks298 (530 points)

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Calculate the standard enthalpy change for the precipitation reaction between lead(II) nitrate and sodium chloride to form lead(II) chloride and sodium nitrate. The balanced chemical equation for the reaction is:Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)

asked Feb 3 in Chemical thermodynamics by FrancescaShe (550 points)

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1 answer 40 views

Calculate the standard enthalpy change (ΔH°) for the following reaction involving the coordination compound [Fe(H2O)6]2+:[Fe(H2O)6]2+(aq) + 2Cl-(aq) → [FeCl2(H2O)4](aq) + 2H2O(l) Given: ΔH°f [FeCl2(H2O)4](aq) = -334 kJ/mol ΔH°f [Fe(H2O)6]2+(aq) = -393 kJ/mol ΔH°f H2O(l) = -286 kJ/mol Note: The superscript ° denotes standard conditions (i.e. 1 atm and 25°C) and the superscript f denotes standard enthalpy of formation.

asked Feb 3 in Chemical thermodynamics by BennettLever (450 points)

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1 answer 37 views

Calculate the standard enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)Given the standard enthalpies of formation are: ΔHf°(H2O(l)) = -285.8 kJ/mol ΔHf°(H2(g)) = 0 kJ/mol ΔHf°(O2(g)) = 0 kJ/mol Assume all reactants and products are at standard state conditions.

asked Feb 3 in Chemical thermodynamics by LanePeacock (490 points)

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Calculate the standard free energy change for the following redox reaction: Balanced Chemical Equation: 2Fe3+(aq) +3H2O2(aq) → 2Fe2+(aq) + 3O2(g) + 6H+(aq)Given data: Standard reduction potential of Fe3+/Fe2+ = +0.77 V Standard reduction potential of H2O2/O2 = +0.70 V

asked Feb 3 in Chemical thermodynamics by AlexisHooten (590 points)

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Calculate the standard enthalpy change for the formation of 2 moles of water vapor (H2O(g)) if the combustion of 1 mole of methane gas (CH4(g)) results in the formation of 2 moles of water vapor and 1 mole of carbon dioxide gas (CO2(g)). Given that the standard enthalpy change of combustion of methane is -890.4 kJ/mol.

asked Feb 3 in Chemical thermodynamics by KEZMeagan45 (350 points)

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