Recent questions in Chemistry

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1 answer 30 views

Ammonia and hydrochloric acid react to form ammonium chloride according to the equation: NH3(g) + HCl(g) ⇌ NH4Cl(s). If a student were to add 0.1 moles of NH4Cl to the mixture at equilibrium and the volume of the container is constant, what will be the new concentration of NH3(g) and HCl(g) in the mixture?

asked Jan 22 in Chemical equilibrium by TorstenDupre (330 points)

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1 answer 45 views

A zinc rod is being placed in a solution containing 0.1 M of copper (II) ions. Calculate the corrosion potential of the zinc rod in a galvanic couple with a standard hydrogen electrode at 25°C.

asked Jan 22 in ElectroChemistry by VictorHoltz (310 points)

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1 answer 59 views

A zinc electrode was kept in a 0.1 M ZnSO4(aq) solution, and a copper electrode was kept in a 0.1 M CuSO4(aq) solution. When 1500 C of electricity was passed through the cell, how many grams of copper were deposited on the cathode? (Assume 100 % efficiency and the Faraday constant is 96500 C/mol)

asked Jan 22 in ElectroChemistry by MerrillAsl57 (570 points)

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1 answer 55 views

A zinc electrode is immersed in a 1.0 M ZnSO4 solution and connected to a platinum electrode that is immersed in a 1.0 M CuSO4 solution. If the measured potential difference of the cell is 1.10 V at 25 °C, what is the polarization of the cell?

asked Jan 22 in ElectroChemistry by EdwardTier7 (550 points)

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1 answer 56 views

A zinc electrode is connected to a copper electrode by a wire in a beaker that has a solution of 0.1 M CuSO4 and 0.1 M ZnSO4. The initial reduction potential of the copper electrode is +0.34 V, and the initial oxidation potential of zinc is –0.76 V. What is the potential difference between the two electrodes at 298 K, and what is the rate of the electrochemical reaction when the cell operates at a current of 2.50 A?

asked Jan 22 in ElectroChemistry by JerryHeaton2 (690 points)

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1 answer 10 views

A voltaic cell consists of a standard hydrogen electrode and a copper electrode in a solution of copper(II) sulfate. The measured cell potential is 0.78 V at 25°C. If the concentration of copper(II) sulfate is 0.1 M, what is the resistance of the electrochemical cell?

asked Jan 22 in ElectroChemistry by Pat220311982 (250 points)

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1 answer 57 views

A student wishes to prepare a buffer solution by adding 0.20 moles of acetic acid (Ka = 1.8 x 10^-5) and 0.20 moles of sodium acetate in 1 liter of solution. The student adds 0.05 moles of hydrochloric acid (HCl) to the solution. Calculate the effect of adding the buffer on the equilibrium position of the acid-base reaction and determine the new pH of the solution.

asked Jan 22 in Chemical equilibrium by ShondaEzell4 (210 points)

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1 answer 56 views

A student wishes to determine the standard reduction potential of an unknown metal electrode in a half-cell. They set up an electrochemical cell using a known standard hydrogen electrode (SHE) as the reference electrode and the unknown metal electrode as the working electrode. A voltmeter is used to measure the potential difference between the two electrodes. The reading is +0.45 V. What is the standard reduction potential of the unknown metal electrode in volts?

asked Jan 22 in Physical Chemistry by CharleneKeen (310 points)

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1 answer 60 views

A student wishes to determine the power output of an electrochemical cell that utilizes a half-reaction of copper oxide reducing to copper and a half-reaction of zinc oxidizing to zinc ions. The initial concentrations of the copper and zinc ions in the cell are 1.00 M and 0.10 M, respectively. The cell operates for 60 minutes at a constant rate of 0.200 A. Given that the standard cell potential is 1.10 V, calculate the power output of the electrochemical cell.

asked Jan 22 in ElectroChemistry by ManuelDeucha (210 points)

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1 answer 71 views

A student wants to synthesize a polymer using the monomer vinyl chloride. The reaction is exothermic and produces a polymer with an average molecular weight of 50,000 g/mol. The enthalpy change of polymerization for this reaction is -121.8 kJ/mol. How much heat is liberated during the polymerization of 1 mol of vinyl chloride?

asked Jan 22 in ThermoChemistry by ShaunCorner (190 points)

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1 answer 54 views

A student wants to produce aluminum oxide (Al2O3) in the lab. Write a balanced chemical equation for the reaction between aluminum and oxygen gas to form aluminum oxide. Calculate how many grams of Al2O3 can be produced from 25 grams of aluminum reacting with excess oxygen gas.

asked Jan 22 in Inorganic Chemistry by CarmaSturges (370 points)

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1 answer 69 views

A student wants to prepare polyethylene using the radical polymerization process. The monomer used is ethylene, and the reaction occurs at a temperature of 60°C. The initiator used is benzoyl peroxide. The student wants to know the enthalpy change that occurs during the polymerization process. How can the student calculate the enthalpy of polymerization using the given information?

asked Jan 22 in ThermoChemistry by JanBallow529 (150 points)

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1 answer 96 views

A student wants to measure the heat of crystallization of sodium acetate trihydrate. The student takes 50 g of sodium acetate trihydrate and dissolves it in 100 ml of water at 70°C. The solution is then allowed to cool to 20°C, during which the sodium acetate trihydrate crystallizes out. The student measures the temperature change during this process and finds that the temperature drops to 45°C. What is the heat of crystallization of sodium acetate trihydrate in kJ/mol?

asked Jan 22 in ThermoChemistry by SherrillThom (330 points)

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1 answer 66 views

A student wants to maximize the production of ammonia from nitrogen and hydrogen gases using the Haber process. Using Le Chatelier's principle, how can the reaction conditions be adjusted to increase the yield of ammonia? Specifically, how can changes in temperature, pressure, and concentration of reactants be used to increase the equilibrium concentration of ammonia?

asked Jan 22 in Chemical reactions by DirkGilruth9 (350 points)

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1 answer 67 views

A student wants to know the equilibrium concentration of hydrogen gas and nitrogen gas at a particular temperature and pressure when they are mixed in a container in a 2:1 ratio. The student also wants to calculate the equilibrium constant of the reaction when nitrogen and hydrogen form ammonia. Can you help the student by designing a step-by-step procedure to find the equilibrium concentrations and equilibrium constant at the given conditions?

asked Jan 22 in Physical Chemistry by GemmaGraff27 (270 points)

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1 answer 59 views

A student wants to know how the equilibrium position of a weak acid such as acetic acid would be affected if they add more acetate ion. If the initial concentration of acetic acid is 0.1 M and initial concentration of acetate ion is 0.05 M. What will be the new concentration of acetate ion necessary to increase the pH of the solution by 0.5 units?

asked Jan 22 in Chemical equilibrium by KandiDempste (210 points)

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1 answer 56 views

A student wants to know how changing the volume affects the position of the equilibrium for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). If the reaction is initially at equilibrium in a 2 L container at 400 K and then the volume is decreased to 1 L, what will be the new concentrations of each gas at equilibrium? (Assume that the pressure remains constant and that the reaction follows the ideal gas law.)

asked Jan 22 in Chemical equilibrium by Margie557251 (450 points)

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1 answer 54 views

A student wants to investigate the thermodynamic properties of a system undergoing a non-equilibrium process. The system is initially at a temperature of 300 K and pressure of 1 atm. A sudden expansion of the system causes the pressure to drop to 0.5 atm while maintaining a constant temperature. Calculate the change in entropy of the system during the process assuming ideal gas behavior.

asked Jan 22 in Physical Chemistry by WiltonBear6 (350 points)

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1 answer 63 views

A student wants to investigate the effect of volume change on the equilibrium position of the reaction 2SO2(g) + O2(g) ⇄ 2SO3(g). The initial equilibrium concentration of SO3 is 0.1 M at a constant temperature. The volume is reduced by half at equilibrium. Calculate the new equilibrium concentrations of SO2, O2 and SO3 assuming the equilibrium constant (Kc) of the reaction remains constant.

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

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1 answer 40 views

A student wants to find the equilibrium constant for the following reaction at a temperature of 298 K:2NO(g) + Cl2(g) ⇌ 2NOCl(g)The student measures the equilibrium concentrations to be [NO] = 0.050 M, [Cl2] = 0.025 M, and [NOCl] = 0.080 M. What is the equilibrium constant (Kc) for the reaction at this temperature?

asked Jan 22 in Chemical reactions by QuyenUxw488 (490 points)

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