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A student conducted an electrochemical reaction using a copper electrode to reduce a solution containing Ag+ ions. The standard reduction potential for Ag+ is 0.80 V and the standard reduction potential for Cu2+ is 0.34 V. The student measured the cell potential to be 0.62 V. Calculate the overpotential of the reaction and determine if the reduction of Ag+ occurs spontaneously.

asked Jan 22 in ElectroChemistry by HildredU3922 (1.9k points)

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1 answer 15 views

A student carried out a chemical reaction in the laboratory and obtained 12 grams of the product. However, the theoretical yield of the product was 15 grams. Calculate the percent yield of the product.

asked Jan 22 in Chemical reactions by WileyBaskerv (2.2k points)

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1 answer 13 views

A student attempted to synthesize 20 grams of a compound, but only ended up with 15 grams of the compound after the reaction. Calculate the percentage yield of the reaction.

asked Jan 22 in Chemical reactions by GraceChaves1 (2.0k points)

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1 answer 36 views

A student attempted to produce 25 grams of product by performing a chemical reaction, but only obtained 18 grams. What was the percent yield for this reaction?

asked Jan 22 in Chemical reactions by JannetteBarr (2.2k points)

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1 answer 60 views

A student adds 0.1 M HCl to a solution containing 0.05 M NaOH. Calculate the effect on the equilibrium position of the system after adding a buffer solution consisting of 0.1 M CH3COOH and 0.1 M CH3COONa. Assume the dissociation constant (Ka) of CH3COOH is 1.8x10^-5.

asked Jan 22 in Chemical equilibrium by GroverRamey (2.2k points)

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A steel pipeline is being used to transport a chemical mixture containing sulfuric acid. Given the concentration of sulfuric acid in the mixture and the surface area of the pipeline, calculate the corrosion rate of the steel pipeline in millimeters per year. Show your calculation and explain the significance of the result.

asked Jan 22 in ElectroChemistry by HenryBorella (2.2k points)

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1 answer 10 views

A steel pipe is in contact with a copper pipe in a galvanic couple, with the steel pipe acting as the anode. The corrosion current density of the steel pipe in the couple is 0.008 mA/cm². Determine the rate of corrosion of the steel pipe, assuming that the density of steel is 7.8 g/cm³ and the thickness of the pipe is 2.5 mm. Also, calculate the time taken for the pipe to corrode completely, assuming an initial mass of 5 kg.

asked Jan 22 in ElectroChemistry by Agustin3989 (1.7k points)

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1 answer 50 views

A steel pipe is connected to a copper pipe in a galvanic corrosion couple where the electrolyte is seawater. The corrosion current density of the steel pipe is 3.2 mA/cm2. If the surface area of the steel pipe is 5 cm2, calculate the total amount of charge transferred per hour. Also, calculate the weight loss of the steel pipe per year due to galvanic corrosion, assuming the density of steel is 7.85 g/cm3.

asked Jan 22 in ElectroChemistry by Aline0805519 (1.8k points)

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1 answer 60 views

A solution of nitrogen dioxide, NO2 gas, at a pressure of 2.50 atm and temperature of 300 K, reacts with oxygen gas, O2, to form nitrogen oxide, NO, and dioxide, NO2. Write the balanced chemical equation for the reaction and determine the equilibrium concentrations of all species if the value of the equilibrium constant, Kc, at 300 K is 4.0 x 10^-4.

asked Jan 22 in Chemical equilibrium by Samira94683 (2.2k points)

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A solution of NaCl was electrolyzed using a current of 2.0 A for 30 minutes. If 0.20 grams of NaCl was consumed in the process, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by FelixTolmer3 (1.9k points)

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1 answer 66 views

A solution of 0.1 M AgNO3 was electrolyzed using a current of 0.5 A for 150 seconds. If 0.15 g of silver was deposited, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by FranY1408156 (2.2k points)

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1 answer 59 views

A solution contains 0.1 M of an unknown ion X. The electrode potential of this ion X is measured to be +0.60 V versus the standard hydrogen electrode (SHE). Calculate the concentration of ion X in the solution using electrochemical methods.

asked Jan 22 in ElectroChemistry by VickeyBatema (1.9k points)

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1 answer 105 views

A solution contains 0.05 mol of Cu^2+ ions. If a current of 0.5 A is passed through this solution for 15 minutes, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by TiaMuirden46 (2.3k points)

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1 answer 10 views

A solution contains 0.05 M AgNO3 and 0.10 M KCl. A silver electrode is dipped in the solution and a potential of 0.53 V is measured against a standard hydrogen electrode. Calculate the concentration of Ag+ ions in the solution.

asked Jan 22 in ElectroChemistry by AntonyKnotts (1.8k points)

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1 answer 34 views

A solution containing two different dye molecules of different sizes (methyl blue and eosin) is kept in a glass tube. Using the knowledge of diffusion and transport phenomena, calculate the time required for the eosin molecules to diffuse to a distance of 10 cm from the source of the solution, if the diffusion coefficient of eosin is known to be 2.5 x 10^-10 m^2/s.

asked Jan 22 in Physical Chemistry by FinleyConsta (2.4k points)

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1 answer 90 views

A solution containing 0.5 moles of potassium dichromate was electrolyzed with a current of 1.5 Amperes for 30 minutes. During the process, the final volume of the solution was found to be 250 mL. Calculate the value of the Faraday constant using this information.

asked Jan 22 in ElectroChemistry by CorneliusChi (1.6k points)

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1 answer 13 views

A solution containing 0.5 M of iron(III) ions and 0.5 M of thiocyanate ions is allowed to reach equilibrium. If the equilibrium constant of the formation of the FeSCN2+ complex ion is 3.0 x 10^3, calculate the concentration of FeSCN2+ complex ion at equilibrium when the initial concentration of thiocyanate ions is doubled.

asked Jan 22 in Chemical equilibrium by BoydHaynes98 (1.9k points)

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1 answer 79 views

A solution containing 0.1 M acetic acid and 0.1 M sodium acetate has a pH of 4.5. If 0.02 moles of hydrochloric acid is added to the solution, what will be the pH of the solution after equilibrium is reached? (Given pKa of acetic acid = 4.76)

asked Jan 22 in Chemical equilibrium by RoderickKyle (2.4k points)

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1 answer 11 views

A small metal block is placed in a beaker containing boiling water. The block initially weighs 50 grams and its temperature is 25°C. After 5 minutes, its weight is 49 grams and its temperature is 80°C. Determine the entropy change of the metal block during this process assuming it to be irreversible.

asked Jan 22 in Physical Chemistry by DelorasGaise (1.9k points)

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1 answer 49 views

A sealed vessel contains a mixture of nitrogen dioxide and dinitrogen tetraoxide gases in equilibrium. If the volume of the container is increased, would the equilibrium shift towards more or less NO2? Calculate the new equilibrium constant at the new volume assuming the pressure and temperature remain constant.

asked Jan 22 in Chemical equilibrium by KreogMoore5 (6.4k points)

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