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Calculate the equilibrium constant (K) for the reaction that occurs when a nickel electrode is placed in a solution containing 1.0 M of nickel ions and 1.0 M of copper ions. The nickel electrode was placed in the solution, and the cell potential was measured to be 0.21 V at 25 °C.

asked Jan 23 in ElectroChemistry by CorneliusU11 (1.7k points)

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Calculate the equilibrium constant (K) for the reaction between copper and silver ions in a galvanic cell at room temperature (25°C), given the following half-reactions and their respective reduction potentials:Cu2+ (aq) + 2e- → Cu (s) E°red = +0.34 VAg+ (aq) + e- → Ag (s) E°red = +0.80 VAlso, if the cell is constructed with a copper electrode and a silver electrode, which electrode will be the cathode and which will be the anode?

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

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Calculate the equilibrium constant (K) for the formation of the complex ion [Fe(SCN)₂⁺] when 3.0 x 10⁻³ moles of Fe(NO₃)₃ and 1.5 x 10⁻³ moles of NaSCN are mixed in a 250 mL solution. The solution shows that the concentration of Fe(SCN)₂⁺ is 1.2 x 10⁻³ M at equilibrium.

asked Jan 23 in Chemical equilibrium by JacquelynDos (1.7k points)

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Calculate the equilibrium constant (K) for the electrochemical reaction: Mg(s) + 2 Ag+(aq) → Mg2+(aq) + 2 Ag(s) Given that the standard reduction potentials for Ag+ and Mg2+ are +0.80 V and -2.37 V, respectively. The concentration of Ag+ is 0.020 M and the concentration of Mg2+ is 0.080 M.

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

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Calculate the equilibrium constant (K$\textsubscript{a}$) for the reaction of acetic acid in aqueous solution if the pH of the solution is 4.76 and the concentration of acetic acid is 0.1 M.

asked Jan 23 in Chemical equilibrium by ElidaHaskins (1.7k points)

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Calculate the equilibrium concentrations of reactants and products for the following reaction at a temperature of 25°C and a pressure of 1 atm:2 NO(g) + Br2(g) ⇌ 2 NOBr(g)Given the initial concentrations are [NO] = 0.20 M, [Br2] = 0.35 M, and [NOBr] = 0.015 M. The equilibrium constant (Kc) for the reaction is 4.8 x 10^2 at 25°C.

asked Jan 23 in Chemical equilibrium by ThaliaSheil (2.0k points)

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Calculate the equilibrium concentration of each species (in mol/L) in a system containing 0.200 M KI and 0.200 M Cl2 that forms KCl and I2 at equilibrium, given that the equilibrium constant (Kc) is 9.0 x 10^-2 at a certain temperature.

asked Jan 23 in Chemical equilibrium by Wilbur29087 (1.8k points)

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Calculate the entropy change when one mole of helium gas is compressed isothermally at 298 K from a volume of 10 L to 2 L. The heat capacity of helium at constant pressure, Cₚ, is 20.8 J/mol*K.

asked Jan 23 in Physical Chemistry by ChanteStroh (1.5k points)

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Calculate the entropy change of the following reaction at 25°C and 1 atm pressure:2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g)Given the standard entropy values are:ΔS°NH3 = 192.5 J/K•molΔS°Cl2 = 223.1 J/K•molΔS°N2 = 191.6 J/K•molΔS°HCl = 186.9 J/K•mol

asked Jan 23 in Chemical thermodynamics by KatieManzi6 (1.6k points)

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Calculate the entropy change of an ideal monatomic gas at 1 atm and 300 K when it expands isothermally to 5 times its initial volume.

asked Jan 23 in Physical Chemistry by Shawn33B4717 (1.9k points)

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Calculate the entropy change for the reaction: 2H2(g) + O2(g) → 2H2O(g)given that the standard molar entropies of H2(g), O2(g), and H2O(g) are 130.7 J/mol.K, 205.0 J/mol.K, and 188.8 J/mol.K, respectively.

asked Jan 23 in Chemical thermodynamics by ZitaHarrell8 (1.8k points)

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Calculate the entropy change for the reaction of 2 moles of methane gas reacting with 4 moles of oxygen gas to form carbon dioxide gas and water vapor at a constant temperature of 298 K. The reaction is balanced and the standard entropy values for methane, oxygen, carbon dioxide, and water vapor are given as -0.242, 205.16, 213.74, and 188.72 J/K/mol, respectively.

asked Jan 23 in Chemical thermodynamics by JackQ7308746 (2.0k points)

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Calculate the entropy change for the following chemical reaction at 25 °C: 2H2(g) + O2(g) → 2H2O(l) Given that the standard molar entropy of H2(g), O2(g), and H2O(l) are 130.68 J/mol·K, 205.03 J/mol·K and 70.01 J/mol·K respectively.

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

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Calculate the entropy change for the combustion of methane at a constant temperature and pressure of 298 K and 1 atm, respectively. The balanced equation for the reaction is:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

asked Jan 23 in Chemical thermodynamics by IsraelSeidel (1.3k points)

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Calculate the entropy change for the combustion of methane (CH4) at 298 K and 1 atm pressure, given the standard molar entropies of CH4, H2O (g), and O2 (g) are 186.3 J/K/mol, 188.7 J/K/mol, and 205.0 J/K/mol, respectively. The balanced chemical equation for the reaction is:CH4 (g) + 2 O2 (g) -> CO2 (g) + 2 H2O (g)

asked Jan 23 in Chemical thermodynamics by BelenPickard (2.3k points)

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Calculate the entropy change (ΔS) for the reaction below at 298 K:2H2(g) + O2(g) → 2H2O(l)Given the standard molar entropy values are:H2(g) = 130.68 J/K molO2(g) = 205.03 J/K molH2O(l) = 69.91 J/K mol

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

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Calculate the entropy change (ΔS) for the combustion of methane gas (CH4) at constant pressure and standard conditions, given the following data: C(s) + O2(g) → CO2(g) ΔS° = -394 J/K·mol 2H2(g) + O2(g) → 2H2O(l) ΔS° = -237 J/K·mol CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH° = -802 kJ/mol

asked Jan 23 in Chemical thermodynamics by MargueriteWa (1.8k points)

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Calculate the entropy change (∆S) when a container of volume 1.0 L is filled with 1.0 mol of ideal gas at a temperature of 300 K and a pressure of 1.0 atm, and then the gas is allowed to expand irreversibly to fill a volume of 2.0 L against a constant external pressure of 0.5 atm at the same temperature.

asked Jan 23 in Physical Chemistry by ChloeBodnar (2.0k points)

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Calculate the entropy change (∆S) for the reaction of 2 moles of solid NH4Cl with 1 mole of NaOH in a coffee cup calorimeter at a constant temperature of 25°C. The reaction takes place in 100 mL of water and produces 2 moles of NH3 and 1 mole of NaCl in solution. Assume that the specific heat capacity of water is 4.18 J/g·K and that the final solution temperature after the reaction is complete is 25°C.

asked Jan 23 in Chemical thermodynamics by GlendaNester (1.8k points)

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Calculate the entropy change (∆S) for the reaction between 2.0 moles of hydrogen gas (H2) and 1.0 mole of oxygen gas (O2) at constant pressure and a temperature of 298 K, given the standard molar entropy values for H2 and O2 to be 130.7 J/K•mol and 205.0 J/K•mol, respectively.

asked Jan 23 in ThermoChemistry by RoderickKyle (2.4k points)

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