Recent questions in Chemistry

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A reaction mixture initially contained 0.1 mol/L of reactant A and 0.2 mol/L of reactant B. When a catalyst was added, the rate of conversion of A and B to the product increased significantly. Calculate the new equilibrium concentration of reactant B if the equilibrium constant of the reaction is 0.1 and the initial equilibrium concentration of the product is 0.05 mol/L. Assume that the catalyst does not change the equilibrium constant.

asked Jan 22 in Chemical equilibrium by Shawn33B4717 (1.9k points)

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A reaction in a container has an equilibrium constant of K = 5.0 x 10^-3 at a particular temperature. If the volume of the container is suddenly decreased by a factor of 2, what will happen to the concentration of each of the reactants and products at equilibrium? Use the reaction below:2A + B ⇌ 3C + D

asked Jan 22 in Chemical equilibrium by PeteWirtz263 (2.1k points)

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1 answer 15 views

A question for the student to solve could be: If a certain equilibrium reaction is exothermic, and the concentration of reactant A is increased while the concentration of product B is decreased, predict the change in the equilibrium constant value (K) and explain your reasoning by applying Le Chatelier's principle.

asked Jan 22 in Chemical reactions by ClairWaite7 (1.8k points)

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A piece of zinc metal is placed in a beaker containing an acidic solution, while a copper electrode is also placed in the same solution. The copper electrode is connected to the positive terminal of a voltmeter, while the zinc electrode is connected to the negative terminal of the voltmeter. If the measured potential between the two electrodes is -0.76 V, what is the corrosion potential of the zinc electrode?

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

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1 answer 70 views

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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1 answer 32 views

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 83 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 116 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 73 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 81 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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1 answer 73 views

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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1 answer 79 views

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 78 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 40 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 69 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 14 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 12 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 112 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 79 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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