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Calculate the pH of a 0.1 M solution of acetic acid with a dissociation constant (Ka) of 1.8 x 10^-5.

asked 5 days ago in Chemical reactions by Xavier496923 (230 points)

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Calculate the standard electrode potential for the redox reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)if the standard electrode potentials for Zn2+/Zn and Cu2+/Cu half-cells are -0.76V and +0.34V, respectively.

asked 5 days ago in Chemical thermodynamics by CliffAachen7 (490 points)

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How does changing the concentration of reactants affect the reaction rate and the resulting yield in the chemical reaction between sodium thiosulfate and hydrochloric acid?

asked 5 days ago in Chemical kinetics by TuyetSticht2 (310 points)

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Calculate the standard electrode potential for the redox reaction that occurs when a silver electrode is placed in a solution containing 0.1 M Ag+ ions and a platinum electrode is placed in a solution containing 0.1 M H+ ions at standard conditions. The reduction half-reaction for Ag+ is Ag+ (aq) + e- → Ag(s), and the reduction half-reaction for H+ is H+ (aq) + e- → 1/2 H2 (g).

asked 5 days ago in Chemical thermodynamics by MontyCockett (430 points)

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Calculate the standard enthalpy change for the neutralization of 50.0 mL of 0.100 M hydrochloric acid with 50.0 mL of 0.100 M sodium hydroxide, assuming that the specific heat capacity of the resulting solution is 4.18 J/g °C and the density of the solution is 1.00 g/mL.

asked 5 days ago in Chemical thermodynamics by MurielC91559 (450 points)

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Calculate the overpotential of an electrochemical cell where Zinc metal is used as an anode and Copper metal as a cathode. The concentration of Zinc ions in the half-cell is 1 M and Copper ions in the half-cell is 0.1 M. The temperature of the system is 25°C. (Given: Standard Reduction Potentials - Zn²⁺ + 2e⁻ → Zn(s) = -0.76 V and Cu²⁺ + 2e⁻ → Cu(s) = +0.34 V)

asked 5 days ago in ElectroChemistry by NestorSeccom (410 points)

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Calculate the standard electrode potential for the reaction Ag+ (aq) + Cu (s) → Ag (s) + Cu2+ (aq) given that the standard electrode potentials for Ag+ (aq) + e- → Ag (s) and Cu2+ (aq) + 2e- → Cu (s) are 0.80 V and 0.34 V respectively.

asked 5 days ago in Chemical thermodynamics by DarbyEastin (210 points)

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Calculate the overpotential of a lead electrode in contact with a solution containing [Pb2+] = 0.001 M when the temperature is 298 K. Given that the standard potential of the Pb2+ / Pb electrode is -0.13 V and the exchange current density is 0.015 A/m2.

asked 5 days ago in ElectroChemistry by JoeyGkg21308 (350 points)

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Calculate the standard enthalpy change for the reaction between 50.0 mL of 0.200 M HCl(aq) and 50.0 mL of 0.300 M NaOH(aq) at 25°C. The heat capacity of the calorimeter is 9.60 J/°C and the temperature change observed is 4.00°C. Also, assume that the density of both solutions is 1.00 g/mL and that the heat capacity and density of the final solution are the same as that of water.

asked 5 days ago in Chemical thermodynamics by InaLewers025 (330 points)

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Calculate the standard enthalpy change for the sublimation of 5 moles of solid iodine (I2) given the following data:- Enthalpy of fusion of iodine = 15.52 kJ/mol- Enthalpy of vaporization of iodine = 41.57 kJ/mol

asked 5 days ago in Chemical thermodynamics by ShelliFogart (370 points)

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1 answer 38 views

What is the effect of changing the concentration of reactants on the rate of a chemical reaction and how does it impact the sustainability of the reaction?

asked 5 days ago in Chemical kinetics by EliBrinkman (330 points)

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What is the effect of changing the concentration of reactants on the rate of reaction and the corresponding safety hazards in a given chemical reaction?

asked 5 days ago in Chemical kinetics by SheilaHoldsw (230 points)

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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 5 days ago in Physical Chemistry by DoreenBurrou (470 points)

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1 answer 22 views

Calculate the standard enthalpy of formation for carbon dioxide (CO2) given the following information: ΔHf° of CO = -26.4 kJ/mol, ΔHf° of O2 = 0 kJ/mol, and ΔH°rxn for the combustion of carbon to form CO2 is -393.5 kJ/mol.

asked 4 days ago in Chemical thermodynamics by Normand57353 (590 points)

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Calculate the standard enthalpy change for the formation of methane (CH4) given the following equations:C(s) + O2(g) ⟶ CO2(g); ΔH = -393.5 kJ/mol2H2(g) + O2(g) ⟶ 2H2O(l); ΔH = -571.6 kJ/mol

asked 5 days ago in Chemical thermodynamics by FosterDibell (230 points)

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1 answer 28 views

Calculate the standard enthalpy change (∆H°) for the following reaction involving liquids:C6H12O6 (s) + 6O2 (g) → 6CO2 (g) + 6H2O (l)

asked 5 days ago in Chemical thermodynamics by Mallory7392 (570 points)

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How does changing the concentration of the reactants affect the rate of reaction and the sustainability of the reaction?

asked 5 days ago in Chemical kinetics by MagnoliaReve (450 points)

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1 answer 31 views

Calculate the polarization potential in an electrochemical cell if the concentration of zinc ions in the anode compartment is 0.5 M, the concentration of copper(II) ions in the cathode compartment is 1.0 M, and the voltage of the cell is 1.1 V. The standard reduction potential of copper(II) ions is +0.34 V and the standard reduction potential of zinc ions is -0.76 V.

asked 5 days ago in ElectroChemistry by Ethel40B2651 (690 points)

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Calculate the standard free energy change for the following redox reaction at 298 K:Mg(s) + 2H+(aq) -> Mg2+(aq) + H2(g)Given: Eºred for Mg2+/Mg = -2.37 V & Eºred for H+/H2 = 0 V.

asked 4 days ago in Chemical thermodynamics by MylesDoherty (550 points)

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1 answer 22 views

Calculate the standard enthalpy change of the dissolution reaction for 5.00 g of NaOH in 100 mL of water, given the molar heat of solution of NaOH as -44.5 kJ/mol.

asked 5 days ago in Chemical thermodynamics by KingP6198366 (410 points)

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