Recent questions in Chemistry

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1 answer 72 views

A student is studying the electrochemical reaction of the metal copper in acidic solution. They measure the current density at different applied potentials and obtain the following data:Potential vs. SHE (V) | Current Density (mA/cm²)---|---0.0 | 0.00.1 | 0.50.2 | 2.00.3 | 5.00.4 | 11.0Using this data, calculate the anodic and cathodic Tafel slopes, and determine the rate constant for the electrochemical reaction.

asked Jan 22 in ElectroChemistry by ZPTCarole74 (510 points)

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1 answer 52 views

A student is studying the electrochemical behavior of a certain metal ion in a solution of varying pH values. They have measured the anodic and cathodic Tafel slopes for the electrode reaction at each pH. The anodic Tafel slope values range from 60 mV/decade to 90 mV/decade, and the corresponding cathodic Tafel slope values range from 50 mV/decade to 70 mV/decade. Is this metal ion undergoing a one-electron or a two-electron transfer reaction? Justify your answer.

asked Jan 22 in ElectroChemistry by ColumbusRebe (830 points)

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1 answer 41 views

A student is studying a chemical reaction that goes to completion in a beaker placed on a heated surface at a constant temperature. After the reaction has come to completion, the student removes the beaker from the heated surface and allows it to cool. Using the principles of non-equilibrium thermodynamics and irreversible processes, how can the student calculate the amount of heat that was transferred during the process? Specifically, what factors must be taken into account in order to accurately calculate the heat transfer?

asked Jan 22 in Physical Chemistry by LouHammons52 (510 points)

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1 answer 58 views

A student is given the electrochemical cell reaction:MnO4-(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l)Calculate the standard potential (in volts) of the cell at 25°C given that the standard reduction potential of MnO4-(aq)/Mn2+(aq) couple and the standard reduction potential of the H+(aq)/H2(g) couple are +1.51 V and 0.00 V, respectively. The concentration of MnO4-(aq) is 0.010 M and that of H+(aq) is 1.00 M.

asked Jan 22 in ElectroChemistry by MistyCordeau (530 points)

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1 answer 55 views

A student is given a sample of an inorganic compound that contains only carbon and hydrogen. The sample has a mass of 0.500 g and, upon combustion, produces 1.442 g of carbon dioxide and 0.589 g of water. Determine the empirical formula of the compound.

asked Jan 22 in Inorganic Chemistry by BarneyWearne (490 points)

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1 answer 47 views

A student is given a mixture of two unknown substances, one organic and one inorganic, and is asked to identify these compounds using mass spectrometry. Can you provide a step-by-step procedure using mass spectrometry to identify the two unknown compounds?

asked Jan 22 in Analytical Chemistry by NamLane0895 (470 points)

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1 answer 8 views

A student is given a lead-acid battery, which has a standard reduction potential of -0.356 V. The battery is undergoing a reaction where Pb(s) + SO4^2-(aq) -> PbSO4(s) + 2e^-. If the concentration of PbSO4 in the anode compartment is 1.15 M and the concentration of PbSO4 in the cathode compartment is 0.55 M, what is the power output of the battery, assuming it has a current of 1.25 A?

asked Jan 22 in ElectroChemistry by Francine68A5 (430 points)

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1 answer 59 views

A student is given a galvanic cell that has a copper electrode and a silver electrode. The concentration of copper ions in the solution surrounding the copper electrode is 1.0 M, and the silver electrode is submerged in a solution of AgNO3 with a concentration of 0.1 M. The cell temperature is 25°C. Calculate the resistance of the electrochemical cell given that the cell is at equilibrium and the cell potential is measured to be 0.46 volts.

asked Jan 22 in ElectroChemistry by ElijahGlaspi (510 points)

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1 answer 51 views

A student is given a galvanic cell consisting of a zinc electrode and a copper electrode. If the concentration of zinc ions in the zinc half-cell is 0.1 M and the concentration of copper ions in the copper half-cell is 1.0 M, what is the corrosion potential of the zinc electrode at standard conditions? (Assume that the standard electrode potential of copper is +0.34 V and that of zinc is -0.76 V.)

asked Jan 22 in ElectroChemistry by KatlynCantam (310 points)

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1 answer 52 views

A student is given a concentration of 0.1 M of CuSO4 and 0.2 M of AgNO3, and is asked to calculate the total resistance of an electrochemical cell with electrodes made of these two solutions separated by a salt bridge. The standard reduction potentials for Cu and Ag are +0.34 V and +0.80 V, respectively. Calculate the total resistance of the cell at 25°C assuming that the cell has a thickness of 1 cm and a cross-sectional area of 10 cm².

asked Jan 22 in ElectroChemistry by KatherinDenn (730 points)

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1 answer 8 views

A student is designing an electrochemical cell using zinc and copper electrodes. The student wants to know the current density (in A/cm²) when the cell operates at a voltage of 1.5 V and a temperature of 25°C. The area of the zinc electrode is 10 cm², and the area of the copper electrode is 5 cm². Assuming a 2:1 ratio for the transfer of electrons between the two electrodes, calculate the current density in the cell.

asked Jan 22 in ElectroChemistry by MagdaAcuna34 (650 points)

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1 answer 51 views

A student is asked to design a distillation column for the separation of a mixture consisting of ethanol and water. The student has to determine the number of theoretical plates required for the column to achieve a product concentration of 95% ethanol, given the feed mixture contains 25% ethanol and 75% water. The student also needs to calculate the amount of steam required for the reboiler to operate at a reflux ratio of 3.5, assuming the total condenser efficiency is 100%.

asked Jan 22 in Chemical engineering by EstebanSerle (470 points)

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1 answer 9 views

A student has a solution of AlF3 with a concentration of [AlF3] = 0.015 M, which is in equilibrium according to the equation: AlF3 (s) ⇌ Al3+ (aq) + 3 F- (aq). Calculate the new equilibrium concentration of F- ions if 0.001 mol of NaF is added to the solution initially at equilibrium. (Ksp of AlF3 = 2.0 x 10^-23, NaF is a common ion with F-)

asked Jan 22 in Chemical equilibrium by RolandCoble3 (490 points)

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1 answer 86 views

A student has a solution of acetic acid (CH3COOH) with a concentration of 0.1 M and wants to calculate the effect of adding sodium acetate (NaCH3COO) with a concentration of 0.05 M on the equilibrium position of the reaction CH3COOH + H2O ↔ CH3COO- + H3O+. Calculate the new equilibrium concentrations of all species and explain the effect of the added common ion on the equilibrium position.

asked Jan 22 in Chemical equilibrium by DesireeRoeme (450 points)

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1 answer 52 views

A student has a sample of an unknown inorganic compound that contains only carbon, oxygen, and nitrogen. They perform a combustion analysis on a 0.230 g sample of the compound, which yields 0.535 g of CO2 and 0.184 g of H2O. Additionally, when the compound is analyzed using a mass spectrometer, the mass spectrum shows a molecular ion peak at m/z = 42. Determine the empirical and molecular formulas of this compound.

asked Jan 22 in Inorganic Chemistry by LazaroShin50 (330 points)

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1 answer 45 views

A student has 5 grams of sulfur and 8 grams of oxygen. When the two are reacted to form sulfur dioxide, which one is the limiting reactant, and how much sulfur dioxide can be produced?

asked Jan 22 in Chemical reactions by MichaelaRick (470 points)

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1 answer 86 views

A student has 20 grams of iron and 40 grams of oxygen. What is the limiting reactant in the reaction between iron and oxygen to form iron oxide (FeO)? How many grams of FeO can be produced assuming complete reaction and no excess reactants?

asked Jan 22 in Chemical reactions by MarcelinoUfz (410 points)

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1 answer 57 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 Dominic1066 (370 points)

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1 answer 86 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 BartLundie14 (570 points)

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1 answer 87 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 AngleaLongwe (180 points)

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