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Calculate the equilibrium constant for the following electrochemical reaction at 298K:$$\ce{2Fe^3+ (aq) + 2I^- (aq) -> 2Fe^2+ (aq) + I2 (s)}$$ Given: Standard reduction potentials: $\ce{Fe^3+ + e^- -> Fe^2+}$ Eº = +0.77V $\ce{2I^- -> I2 + 2e^- }$ Eº = +0.54V

asked Jan 23 in ElectroChemistry by Ben56061281 (1.4k points)

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Calculate the equilibrium constant for the following electrochemical cell reaction at 25°C:Cu(s) + 2 Ag+(aq) --> Cu2+(aq) + 2 Ag(s)Given the standard reduction potentials are:Cu2+(aq) + 2 e- → Cu(s) E°red = +0.34 VAg+(aq) + 1 e- → Ag(s) E°red = +0.80 V

asked Jan 23 in ElectroChemistry by DeenaKuhn606 (2.0k points)

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Calculate the equilibrium constant for the electrochemical reaction: Zn(s) + 2H^+(aq) → Zn^2+(aq) + H2(g) when the concentration of Zn^2+ is 0.25 M, [H^+] is 2.5 × 10^-3 M, and the pressure of H2 is 0.8 atm at 298 K.

asked Jan 23 in ElectroChemistry by GiselleDange (1.6k points)

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Calculate the equilibrium constant for the electrochemical cell reaction given below, if the standard reduction potential for the reduction of Fe3+ ion is -0.771 V and for the reduction of Ag+ ion is +0.799 V. Fe3+ + 3e- → Fe (s) E° = -0.771 VAg+ + e- → Ag (s) E° = +0.799 V

asked Jan 23 in ElectroChemistry by JonasOql0066 (1.5k points)

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Calculate the equilibrium constant for a reaction involving a weak oxidizing agent where the concentration of the oxidizing agent is 0.1 M and the concentration of the reduced species is 0.05 M at equilibrium. The balanced chemical equation of the reaction is given as follows:OX + 2 e- ⇌ REDwhere OX is the weak oxidizing agent and RED is the reduced species.

asked Jan 23 in Chemical equilibrium by LeesaJ55672 (1.9k points)

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Calculate the equilibrium constant at 25°C for the reaction: CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) If at equilibrium, the concentration of CO is 0.10 M, H2 is 0.20 M, CH4 is 0.015 M and H2O is 0.035 M.

asked Jan 23 in Chemical equilibrium by IsabellaOcto (1.9k points)

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Calculate the equilibrium constant (Kc) of the reaction below at 25°C with and without a catalyst and determine the effect of the catalyst on the equilibrium position.N2(g) + 3H2(g) ⇄ 2NH3(g)

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

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Calculate the equilibrium constant (Kc) of the chemical reaction: 2NOCl(g) ⇌ 2NO(g) + Cl2(g) where the concentration of NOCl is 0.5 M, NO is 0.2 M, and Cl2 is 0.1 M at equilibrium at a certain temperature.

asked Jan 23 in Chemical reactions by OnitaLoftus1 (2.3k points)

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Calculate the equilibrium constant (Kc) for the reaction: 2A(g) + B(g) ⇌ C(g) + D(g), if the concentration of A is 0.25 M, the concentration of B is 0.10 M, the concentration of C is 0.30 M and the concentration of D is 0.20 M at equilibrium.

asked Jan 23 in Chemical thermodynamics by ElvaL9406057 (2.3k points)

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Calculate the equilibrium constant (Kc) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) if the equilibrium concentration of nitrogen (N2) is 0.025 M, hydrogen (H2) is 0.10 M, and ammonia (NH3) is 0.015 M.

asked Jan 23 in Chemical reactions by DXGMilagros4 (1.9k points)

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Calculate the equilibrium constant (Kc) for the reaction between nitrogen gas (N2) and hydrogen gas (H2) to form ammonia gas (NH3) at a temperature of 400 K. The reaction is written as follows: N2(g) + 3H2(g) ⇌ 2NH3(g) Given the equilibrium concentrations are [N2] = 0.10 M, [H2] = 0.20 M, and [NH3] = 1.0 M.

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

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Calculate the equilibrium constant (Kc) for the reaction between iodine (I2) and potassium iodide (KI) in an aqueous solution, given that at equilibrium, the concentration of iodine is 0.008 M and the concentration of potassium iodide is 0.15 M. The balanced equation for the reaction is given below:I2 (aq) + 2KI (aq) ⇌ 2K+ (aq) + 2I- (aq)

asked Jan 23 in Chemical equilibrium by FawnSharrow (1.9k points)

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Calculate the equilibrium constant (Kc) for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) if at a certain temperature, the initial concentrations of SO2, O2, and SO3 are 0.1 M, 0.2 M, and 0 M, respectively. The equilibrium concentrations of SO2 and SO3 are both 0.05 M. Assume the reaction takes place in a closed system at constant pressure.

asked Jan 23 in Chemical thermodynamics by OnaSchnell25 (1.8k points)

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Calculate the equilibrium constant (Kc) for the following reaction at 300 K: N2(g) + 3 H2(g) ↔ 2 NH3(g) given that at equilibrium, the concentration of N2 is 0.12 M, H2 is 0.20 M, and NH3 is 0.16 M.

asked Jan 23 in Chemical equilibrium by Dwain5313275 (2.5k points)

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Calculate the equilibrium constant (Kc) for the following gas-phase reaction at 298 K: N2(g) + O2(g) ⇌ 2NO(g) where the initial concentrations of N2, O2, and NO are 0.100 M, 0.050 M, and 0.000 M respectively.

asked Jan 23 in Chemical equilibrium by Cameron54A25 (1.9k points)

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Calculate the equilibrium constant (Kc) for the following chemical reaction at 25°C, given that the concentrations of reactant A and product B are 0.05 M and 0.10 M, respectively:A(s) + 2B(g) ⇌ 3C(g) The equilibrium concentration of compound C is found to be 0.15 M.

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

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Calculate the equilibrium constant (Kc) at 298 K for the reaction: 2 NH3(g) ⇌ N2(g) + 3 H2(g) given that the equilibrium concentration of NH3 is 0.20 M, N2 is 0.025 M, and H2 is 0.060 M.

asked Jan 23 in Chemical thermodynamics by StuartCarson (2.4k points)

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Calculate the equilibrium constant (Kc) at 25°C for the following redox reaction involving a weak oxidizing agent: H2O2(aq) + 2I^-(aq) + 2H^+(aq) ⇌ I2(aq) + 2H2O(l)

asked Jan 23 in Chemical equilibrium by AhmadEho9450 (1.6k points)

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Calculate the equilibrium constant (K) of the electrochemical reaction below at 298K:Fe(s) + Cu2+(aq) ⇌ Fe2+(aq) + Cu(s) Given that at standard state (1 atm and 298K) the standard reduction potentials of Fe2+(aq)/Fe(s) and Cu2+(aq)/Cu(s) are -0.44 V and +0.34 V, respectively.

asked Jan 23 in ElectroChemistry by LibbyHollera (2.4k points)

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Calculate the equilibrium constant (K) of the electrochemical reaction below at 25°C: 2AgCl(s) + H2(g) <--> 2Ag(s) + 2HCl(aq) Given: E°AgCl/Ag = 0.22 V E°HCl/H2 = 0.00 V Kw = 1.0 x 10^-14 at 25°C Standard Hydrogen Electrode (SHE) has E° = 0.00 V

asked Jan 23 in ElectroChemistry by QJXClarice2 (2.5k points)

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