Recent questions in Chemistry

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Calculate the standard electrode potential (E°) for the redox reaction of the following half-reactions:Cu2+(aq) + 2e- → Cu(s) E° = +0.34 VFe3+(aq) + e- → Fe2+(aq) E° = +0.77 V

asked Feb 3 in Chemical thermodynamics by BradyBassett (2.0k points)

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1 answer 106 views

Calculate the standard electrode potential (E°) for the reaction below at 298K using the standard reduction potentials given:2H⁺(aq) + 2e⁻ → H₂(g) E°= 0.00VFe³⁺(aq) + e⁻ → Fe²⁺(aq) E°=+0.77V 2H⁺(aq) + Fe³⁺(aq) → H₂(g) + Fe²⁺(aq)

asked Feb 3 in Chemical thermodynamics by WallaceUpsha (2.4k points)

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1 answer 136 views

Calculate the standard change in entropy for the reaction below using the given standard enthalpy and temperature information: 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g) ΔH° = -770.2 kJ T = 298 K

asked Feb 3 in Inorganic Chemistry by KellyStreeto (1.6k points)

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1 answer 127 views

Calculate the standard cell potential of the following electrochemical cell: Ag(s) │ AgCl(s) │ Cl^-(aq, 0.040 M) ‖ Cu^2+(aq, 0.020 M) │ Cu(s) at 298 K. The reduction potential of AgCl/Ag couple is +0.22 V and the reduction potential of Cu^2+/Cu couple is +0.34 V.

asked Feb 3 in Physical Chemistry by XHQMikel9006 (2.0k points)

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1 answer 176 views

Calculate the standard cell potential of the following electrochemical cell at 298 K, given the half-reactions and their standard reduction potentials in brackets:Cu(s) | Cu^2+(0.001 M) || Ag+(0.1 M) | Ag(s)

asked Feb 3 in Physical Chemistry by GingerJ92570 (1.6k points)

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1 answer 132 views

Calculate the standard cell potential for the following electrochemical reaction: Zn (s) + 2 Ag+ (aq) → Zn2+ (aq) + 2 Ag (s)Given: Standard Reduction Potentials are E°Zn2+ = -0.76 V, E°Ag+ = 0.80 V.

asked Feb 3 in ElectroChemistry by DaisyThwaite (1.9k points)

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1 answer 140 views

Calculate the standard cell potential (E°) for the following electrochemical cell:Zn(s) | Zn2+(aq, 0.100M) || Cr3+(aq, 0.050M) | Cr(s)Given: E°cell (Zn2+/Zn) = -0.76 VE°cell (Cr3+/Cr) = -0.74 V

asked Feb 3 in Physical Chemistry by GavinMott60 (1.8k points)

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1 answer 152 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 Vance58E9387 (1.9k points)

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1 answer 162 views

Calculate the specific heat capacity of water if it absorbs 400 J of energy and its temperature rises by 20°C.

asked Feb 3 in Chemical thermodynamics by DKGStacy090 (2.4k points)

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1 answer 133 views

Calculate the resistance of an electrochemical cell with a cell potential of 1.5 V and current flow of 0.25 A when the concentration of copper(II) ions in the cathode compartment is 0.25 M and the concentration of zinc ions in the anode compartment is 0.50 M. The cell has two electrodes made of platinum and the temperature is 25°C. (Assume the transfer of electrons and ions is 100% efficient.)

asked Feb 3 in ElectroChemistry by EvieMerideth (2.3k points)

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1 answer 161 views

Calculate the resistance of an electrochemical cell given the following parameters: - The cell has a total area of 50 cm² and a separation between the electrodes of 2 cm.- The electrolyte solution has a conductivity of 2.5 × 10⁻⁴ S/cm and a temperature of 25°C.- The electrode on the left side of the cell is made of platinum and has a surface area of 25 cm². The electrode on the right side is made of silver and has a surface area of 25 cm².- The distance between each electrode and the solution is 0.5 cm.

asked Feb 3 in ElectroChemistry by JosetteSarto (2.0k points)

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1 answer 138 views

Calculate the resistance of an electrochemical cell constructed by using a copper electrode in a 1M copper (II) sulfate solution and a zinc electrode in a 1M zinc sulfate solution. The measured potential difference of the cell is 1.45 volts. The area of each electrode is 10cm² and the length of wire connecting the electrodes is 30cm with a cross-sectional area of 1 mm². The conductivity of copper (II) sulfate and zinc sulfate solutions at the given concentration is 98.3% and 89.9% respectively. What is the resistance (in ohms) of the electrochemical cell?

asked Feb 3 in ElectroChemistry by JeremyCanady (2.1k points)

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1 answer 173 views

Calculate the resistance of a electrochemical cell at 25°C if the standard reduction potential of the anode is -1.36 V and the standard reduction potential of the cathode is +0.40 V. The solution contains 0.1 M CuSO4 and 0.01 M ZnSO4. The distance between the two electrodes is 5 cm and the cross-sectional area of each electrode is 2.5 cm².

asked Feb 3 in ElectroChemistry by TarenSalmond (1.8k points)

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1 answer 157 views

Calculate the reaction quotient, Qc, for the reaction: 2 NO2 (g) + Cl2 (g) ⇌ 2 NO2Cl (g)At a certain temperature, the concentrations were found to be: [NO2] = 0.15 M, [Cl2] = 0.20 M, and [NO2Cl] = 0.10 M.Is the reaction at equilibrium? If not, which direction would the reaction proceed to reach equilibrium?

asked Feb 3 in Chemical thermodynamics by ErickAshton2 (1.9k points)

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1 answer 106 views

Calculate the reaction quotient, Qc, for the following reaction:2NO2(g) + 7H2(g) → 2NH3(g) + 4H2O(g)at a temperature of 300 K and a pressure of 0.5 atm for each gas species. The equilibrium constants, Kc, at the same temperature and pressure are:Kc = 0.0080 for the reverse reactionKc = 7.2 × 10^-7 for the forward reaction

asked Feb 3 in Chemical thermodynamics by SvenMcConnel (1.3k points)

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1 answer 152 views

Calculate the reaction quotient, Q, for the following reaction at room temperature:$$\ce{CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g)}$$Given:- Partial pressure of methane, $\ce{CH4}$ = 0.25 atm- Partial pressure of oxygen, $\ce{O2}$ = 0.75 atm- Partial pressure of carbon dioxide, $\ce{CO2}$ = 0.0 atm- Partial pressure of water vapor, $\ce{H2O(g)}$ = 0.0 atmUse Q to determine if the reaction is at equilibrium, or if it will shift towards the products or reactants to reach equilibrium.

asked Feb 3 in Chemical thermodynamics by BarrettGriff (2.0k points)

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1 answer 139 views

Calculate the reaction quotient, Q, for the following balanced chemical reaction at 298 K:2NO(g) + O2(g) ⇌ 2NO2(g)Given that the initial concentrations of NO, O2 and NO2 are 0.10 M, 0.15 M and 0.05 M, respectively.

asked Feb 3 in Chemical thermodynamics by LidiaBautist (1.4k points)

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1 answer 95 views

Calculate the reaction quotient Q for the chemical reaction below using the given concentrations of reactants and products at a temperature of 25°C:2H2(g) + O2(g) -> 2H2O(g)[H2] = 0.10 M, [O2] = 0.05 M, [H2O] = 0.08 M.

asked Feb 3 in Chemical thermodynamics by RosalineRigg (1.9k points)

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1 answer 141 views

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 JulianKnetes (2.0k points)

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1 answer 136 views

Calculate the reaction quotient (Qc) for the following reaction at 25°C, given the concentration of reactants and products:2NO2(g) + F2(g) ⇌ 2NO2F(g)[NO2] = 0.30 M, [F2] = 0.40 M, [NO2F] = 0.60 M.Is the reaction at equilibrium? If not, in which direction will the reaction proceed to achieve equilibrium?

asked Feb 3 in Chemical thermodynamics by LizaSwenson (1.7k points)

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