Recent questions in Chemistry

0 votes

1 answer 80 views

A student formed 25 grams of carbon dioxide through a chemical reaction. If the theoretical yield of carbon dioxide is 30 grams, what is the percent yield of the reaction?

asked Jan 22 in Chemical reactions by KyleSchlemme (2.1k points)

0 votes

1 answer 101 views

A student conducted an experiment to produce copper sulfate using a known amount of copper oxide and sulfuric acid. The expected yield was 30 grams of copper sulfate, but the student obtained only 25 grams. What is the percent yield of the reaction?

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

0 votes

1 answer 107 views

A student conducted an experiment to calculate the Faraday constant using a silver-copper voltaic cell. The masses of the copper and silver electrodes were 4.023g and 4.721g respectively. The cell was run for 782 seconds at a constant current of 0.250A. Calculate the value of the Faraday constant for this experiment.

asked Jan 22 in ElectroChemistry by Jaqueline50I (2.0k points)

0 votes

1 answer 109 views

A student conducted an electrolysis experiment using a current of 2 amperes for 30 minutes with a copper sulfate solution. What is the mass of copper deposited on the cathode? The atomic weight of copper is 63.546 g/mol and the Faraday constant is 96,485 C/mol.

asked Jan 22 in ElectroChemistry by TawnyaI60415 (1.4k points)

0 votes

1 answer 71 views

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)

0 votes

1 answer 39 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)

0 votes

1 answer 38 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)

0 votes

1 answer 40 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)

0 votes

1 answer 74 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)

0 votes

1 answer 37 views

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)

0 votes

1 answer 13 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)

0 votes

1 answer 53 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)

0 votes

1 answer 75 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)

0 votes

1 answer 84 views

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)

0 votes

1 answer 69 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)

0 votes

1 answer 73 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)

0 votes

1 answer 118 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)

0 votes

1 answer 41 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)

0 votes

1 answer 36 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)

0 votes

1 answer 98 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)

Categories