Recent questions in Chemistry

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Calculate the formal charge of nitrogen in the molecule of ammonia (NH3) assuming it has single covalent bonds.

asked Jan 23 in Chemical bonding by EarleFrost99 (410 points)

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1 answer 46 views

Calculate the formal charge of nitrogen in the molecule NO₃⁻.

asked Jan 23 in Chemical bonding by RenaChesser8 (710 points)

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1 answer 55 views

Calculate the formal charge of nitrogen in the molecule NO3-.

asked Jan 23 in Chemical bonding by GonzaloHowit (590 points)

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1 answer 39 views

Calculate the formal charge of each atom in the molecule SO3.

asked Jan 23 in Chemical bonding by EdithColebat (530 points)

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1 answer 49 views

Calculate the final temperature when 25 grams of aluminum at 80°C is placed in 100 grams of water at 25°C. The specific heat capacity of aluminum is 0.90 J/g°C and the specific heat capacity of water is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by BrittnyKenne (390 points)

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1 answer 51 views

Calculate the Faraday constant for a half-cell reaction in which the electrode potential is 0.32 V and one mole of electrons are exchanged during the reaction. Express your answer in units of coulombs per mole.

asked Jan 23 in ElectroChemistry by GinaAragon71 (350 points)

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1 answer 39 views

Calculate the extent of polarization for a cell in which a copper electrode is coupled with a silver electrode at 25°C. The copper electrode has a potential of -0.34 V and the silver electrode has a potential of 0.80 V. The initial concentration of copper ions and silver ions in the solution are 0.001 M and 0.01 M, respectively. The total resistance of the cell (including both the electrolyte and the external circuit) is 10 ohms. Assume that the transfer coefficient for both the copper and silver ions is 0.5, and the Faraday constant is 96,485 C/mol.

asked Jan 23 in ElectroChemistry by EliPicard920 (290 points)

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1 answer 51 views

Calculate the expected boiling point of lithium fluoride (LiF) using its experimental melting point and the heat of fusion, assuming it behaves ideally.

asked Jan 23 in Inorganic Chemistry by CasimiraTran (530 points)

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1 answer 62 views

Calculate the exchange current density of a copper-copper(II) ion electrode at 25 °C, given that the standard potential of the electrode is +0.34 V versus the standard hydrogen electrode and the transfer coefficient of the electrode reaction is 0.5.

asked Jan 23 in ElectroChemistry by Philip176831 (390 points)

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1 answer 39 views

Calculate the exchange current density for the redox reaction: Fe2+ + Cr2O72- + 14H+ → 2Fe3+ + 2Cr3+ + 7H2O Given that the standard potential for the reaction at 25°C is 1.33 V, the gas constant is 8.314 J/mol K, and the temperature is 298 K.

asked Jan 23 in ElectroChemistry by DanielleBouc (490 points)

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1 answer 40 views

Calculate the exchange current density for a Zinc electrode immersed in a solution containing 0.1 M Zinc ions at 25 degrees Celsius, given that the standard potential of the Zinc half-reaction is -0.76 V and the transfer coefficient is 0.5. (Assume concentration polarization effects to be negligible.)

asked Jan 23 in ElectroChemistry by JolieTristan (460 points)

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1 answer 8 views

Calculate the exchange current density for a zinc electrode immersed in a 1.0 M solution of zinc sulfate at 25°C when the overpotential is 0.05 V. The standard reduction potential for the Zn2+/Zn couple is -0.76 V. The transfer coefficient is 0.5. Assume that the concentration of the electrolyte does not change significantly during the reaction.

asked Jan 23 in ElectroChemistry by SilkeVelasqu (450 points)

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1 answer 49 views

Calculate the exchange current density for a redox reaction where the standard potential is 0.7 V, and the transfer coefficient is 0.5, given that the rate constant for the reaction is 5 × 10^-7 mol/cm^2*s.

asked Jan 23 in ElectroChemistry by BernadetteFi (390 points)

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1 answer 58 views

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 TabathaTedbu (510 points)

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1 answer 10 views

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 MirandaJephc (410 points)

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1 answer 53 views

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 YongSheehy6 (350 points)

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1 answer 55 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 ImaSchardt52 (390 points)

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1 answer 63 views

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 JorjaIsbell (450 points)

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1 answer 51 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 HamishChappe (530 points)

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1 answer 11 views

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 ElmerAnderse (470 points)

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