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A piece of metal with a mass of 15 grams initially at 25°C is placed in 50 mL of water at 80°C. After the metal has reached thermal equilibrium with the water, its temperature is 30°C. Calculate the specific heat capacity of the metal.

asked Jan 22 in ThermoChemistry by IsabellFrome (2.1k points)

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A metal rod of 3 cm diameter and 20 cm length is placed in a solution of hydrochloric acid with a pH of 2 at 25°C. The metal has a critical pitting temperature of 40°C and a standard electrode potential of -0.44V. Assuming that the rod is polarized to a potential of -0.50V, what is the corrosion current density (in mA/cm²) of the metal in the given environment?

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

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A metal rod made of iron is coupled with a zinc rod in an aqueous medium. If the corrosion potential of the iron rod is -0.44 V and that of the zinc rod is -0.76 V, calculate the corrosion current density of the iron rod when coupled with the zinc rod at 25°C. The polarization resistance of the iron rod is 880 Ωcm².

asked Jan 22 in ElectroChemistry by Damon31M1921 (2.4k points)

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1 answer 68 views

A metal electrode immersed in a solution is used to convert a chemical reaction into an electric current. The electrode potential is measured as the voltage difference between the metal and the solution. The cathodic and anodic Tafel slopes are then calculated in order to determine the rate of the chemical reaction occurring at the electrode. Given a metal electrode immersed in a 0.1 M solution of AgNO3, the cathodic and anodic Tafel slopes are determined to be 120 mV/decade and 110 mV/decade, respectively. Calculate the exchange current density for the reaction occurring at the electro

asked Jan 22 in ElectroChemistry by LynwoodLundg (1.5k points)

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1 answer 103 views

A laboratory made a buffer solution by mixing 25 mL of 0.10 M acetic acid (Ka = 1.8 x 10^-5) with 15 mL of 0.20 M sodium acetate solution. Calculate the pH of the buffer solution assuming both the acid and the acetate ions are completely dissociated.

asked Jan 22 in Chemical reactions by OrenDarwin6 (1.9k points)

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1 answer 60 views

A laboratory assistant is asked to prepare a buffer solution with a pH of 7.10 using acetic acid (CH3COOH) and sodium acetate (NaCH3COO). If the laboratory assistant has 250 mL of 0.20 M acetic acid, how many grams of NaCH3COO will be needed to make the buffer solution?

asked Jan 22 in Chemical reactions by ReinaldoMunz (1.2k points)

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1 answer 71 views

A gas-phase reaction A ⇌ B is known to have a rate constant of 0.05 L/mol/s at 300 K. If the initial concentration of A is 0.1 M and the system reaches equilibrium after 2 minutes, what is the concentration of B at equilibrium? (Assume constant pressure and ideal gas behavior)

asked Jan 22 in Physical Chemistry by RemonaPinto (1.8k points)

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A gas phase reaction occurs according to the following equation: A(g) + 2B(g) -> C(g) + D(g)The reaction is carried out at a total pressure of 2 atm and at 298 K. The initial concentrations of A and B are 0.1 M and 0.2 M, respectively. The rate of formation of C is measured to be 0.02 M/s. What is the rate of disappearance of B?

asked Jan 22 in Physical Chemistry by EmanuelWaldo (2.0k points)

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A gas mixture contains equal parts of hydrogen and helium gases in a container at a temperature of 300 K. Determine the total internal energy of the gas mixture using the grand canonical ensemble model.

asked Jan 22 in Physical Chemistry by HermineOverb (2.1k points)

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1 answer 59 views

A gas is contained in a cylinder at a pressure of 1 atm and a temperature of 25°C. The cylinder is fitted with a piston that can be moved to change the volume. The gas is allowed to expand irreversibly to a final pressure of 0.5 atm, and the temperature is kept constant. Calculate the work done by the system, and determine if the process is endothermic or exothermic.

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

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1 answer 37 views

A galvanic cell has a standard emf of 1.10 V at 298 K. If this cell runs for 25 minutes with a constant current of 0.25 A, what is the amount of energy produced in joules? (Assume the cell is operating under standard conditions.)

asked Jan 22 in ElectroChemistry by ErikaStephen (2.4k points)

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1 answer 66 views

A galvanic cell consists of a standard hydrogen electrode (SHE) as the cathode and a copper electrode as the anode. The measured potential difference between the two electrodes is 1.23 V. Using Tafel analysis, calculate the anodic and cathodic Tafel slopes for the copper electrode.

asked Jan 22 in ElectroChemistry by ConnieSmothe (2.4k points)

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1 answer 12 views

A droplet of water weighing 0.2 grams is placed on the surface of a perfectly clean glass plate. The diameter of the droplet is measured to be 5 mm. Calculate the surface tension of water in dynes/cm.

asked Jan 22 in Surface Chemistry by MellisaOlivo (1.9k points)

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1 answer 9 views

A cylinder with a volume of 2.5 L contains 1.5 moles of an ideal gas at a pressure of 5 atm. The gas is allowed to expand isothermally against a constant external pressure of 1 atm until the volume doubles. Calculate the work done by the gas during the expansion process.

asked Jan 22 in Physical Chemistry by JoyEdge34400 (2.3k points)

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1 answer 89 views

A current of 2.5 amperes was passed through molten silver chloride for 5 hours. What mass of silver metal will be deposited? (The atomic mass of silver = 107.87 g/mol)

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

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1 answer 59 views

A copper wire is exposed to a solution containing 0.2 M NaCl. The corrosion rate of the wire is found to be 5.8 microAmp/cm². Calculate the corrosion current density of the copper wire in the given environment.

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

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1 answer 50 views

A copper rod with a surface area of 5 cm² is coupled with an iron rod with a surface area of 10 cm² to form a galvanic cell. When the circuit is closed, the current flows for 2 hours and the weight loss of the iron rod was found to be 0.58 g. Determine the corrosion rate of the iron rod in millimeters per year (mm/yr) assuming a density of 7.86 g/cm³ for the iron.

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

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1 answer 67 views

A copper electrode is placed in a 1.0 M Cu(NO3)2 solution while a silver electrode is placed in a 1.0 M AgNO3 solution. If the cell potential is measured to be 0.74 V at standard state conditions, what is the equilibrium constant for the reaction Cu(s) + 2Ag+(aq) ⇌ Cu2+(aq) + 2Ag(s)?

asked Jan 22 in ElectroChemistry by EmelyColton2 (1.6k points)

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1 answer 10 views

A copper electrode is immersed in a 0.1M solution of CuSO4 and a zinc electrode is immersed in 0.1M solution of ZnSO4. Both the solutions are connected with a salt bridge. If the standard reduction potentials of Cu2+/Cu and Zn2+/Zn are +0.34V and -0.76 V respectively, calculate the potential difference between the two electrodes at 25°C.

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

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1 answer 100 views

A container initially contains 0.10 mol of NOBr, 0.10 mol of NO, and 0.10 mol of Br2. If the system reaches equilibrium and the concentration of NOBr is found to be 0.075 M at that point, calculate the concentration of NO and Br2 at equilibrium.

asked Jan 22 in Chemical equilibrium by JodieGartrel (1.8k points)

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