Recent questions in Chemistry

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Calculate the exchange current density for a metal electrode immersed in a 1 M solution of its corresponding ions. The standard rate constant for the reaction is 6.3 x 10^-5 cm/s and the concentration of the electrons in the electrode is 5 x 10^23 atoms/cm^3. Additionally, assume the temperature is 25°C and the Faraday constant is 96,500 C/mol.

asked Jan 23 in ElectroChemistry by Leif76792351 (2.0k points)

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Calculate the exchange current density at the interface between a silver electrode and an aqueous solution of silver ions, given that the standard reduction potential for the Ag+/Ag half-cell is +0.80 V, the concentration of Ag+ in the solution is 0.025 M, and the temperature is 25°C.

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

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Calculate the exchange current density at the cathode of a lithium-ion battery if the temperature of the battery is 25 °C, the standard potential of

asked Jan 23 in ElectroChemistry by OnitaLoftus1 (2.3k points)

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1 answer 61 views

Calculate the equilibrium constant, Kc, for the reaction:2SO2(g) + O2(g) ⇌ 2SO3(g) at a temperature of 600 K, given that the initial concentrations of SO2, O2, and SO3 were 0.025 M, 0.014 M, and 0 M, respectively, and at equilibrium [SO2] = 0.015 M, [O2] = 0.008 M, and [SO3] = 0.025 M.

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

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Calculate the equilibrium constant, Kc, for the reaction below at 25°C, if the concentration of CO2 is 0.10 M, the concentration of H2 is 0.20 M, and the concentration of CO is 0.30 M.CO2(g) + H2(g) ⇌ CO(g) + H2O(g)

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

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1 answer 56 views

Calculate the equilibrium constant, Kc, for the reaction below at 25°C if the concentration of CO2 is 1.2 M, the concentration of H2 is 0.8 M and the concentration of CO is 0.6 M.CO2(g) + H2(g) ⇌ CO(g) + H2O(g)

asked Jan 23 in Chemical equilibrium by JanieCorso7 (1.9k points)

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Calculate the equilibrium constant, Kc, at 298 K for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g) when the initial concentrations of SO2, O2, and SO3 are 0.100 M, 0.200 M, and 0.300 M, respectively.

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

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1 answer 61 views

Calculate the equilibrium constant, Ka, for the dissociation of a weak acid HA with an initial concentration of 0.10 M that ionizes to form H+ and A-. At equilibrium, the concentration of H+ is found to be 1.0 x 10^-5 M and the concentration of A- is 0.09 M.

asked Jan 23 in Chemical equilibrium by Sterling80B (2.1k points)

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1 answer 65 views

Calculate the equilibrium constant, K, for the electrochemical reaction below, given the standard reduction potentials at 298 K:2 H+ (aq) + 2 e- → H2 (g) E° = 0.00 VFe3+ (aq) + e- → Fe2+ (aq) E° = +0.771 V

asked Jan 23 in ElectroChemistry by TroyPurton77 (1.9k points)

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Calculate the equilibrium constant for the reaction: 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) if at equilibrium the concentrations are [NOCl] = 0.050 M, [NO] = 0.030 M, and [Cl2] = 0.020 M.

asked Jan 23 in Chemical equilibrium by SNBBernd7967 (2.3k points)

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1 answer 73 views

Calculate the equilibrium constant for the reaction that occurs when a copper electrode is placed in a solution of 0.1 M copper(II) sulfate and connected to a standard hydrogen electrode. The cell potential at standard conditions is observed to be 0.34 V. (Hint: Use the Nernst equation to relate the cell potential to the equilibrium constant.)

asked Jan 23 in ElectroChemistry by YvetteLink0 (2.0k points)

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1 answer 73 views

Calculate the equilibrium constant for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g), given that the concentrations at equilibrium are [SO2] = 0.20 M, [O2] = 0.30 M and [SO3] = 0.50 M.

asked Jan 23 in Chemical equilibrium by ErickB565479 (1.8k points)

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1 answer 66 views

Calculate the equilibrium constant for the following electrochemical reaction at a temperature of 25°C:$$\ce{Co^{2+} + 2e^- <=> Co(s)}$$Given that the standard reduction potential for the half-reaction is $-0.28\,\text{V}$ and the concentration of $\ce{Co^{2+}}$ is $0.1\,\text{M}$.

asked Jan 23 in ElectroChemistry by Shawn33B4717 (1.9k points)

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1 answer 65 views

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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1 answer 51 views

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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1 answer 69 views

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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1 answer 56 views

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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1 answer 60 views

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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1 answer 62 views

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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1 answer 70 views

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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