Recent questions in Chemistry

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Calculate the reaction quotient (Qc) for the following chemical reaction at 25°C: 2SO2(g) + O2(g) ⟶ 2SO3(g)Given the following concentration values:[SO2] = 0.1 M[O2] = 0.05 M[SO3] = 0.3 MWhat is the reaction quotient Qc for this reaction? Is the reaction at equilibrium? If not, in which direction will the reaction proceed to reach equilibrium?

asked Feb 3 in Chemical thermodynamics by MerryGoodsel (1.9k points)

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1 answer 131 views

Calculate the reaction quotient (Qc) for the chemical equation:2NO(g) + O2(g) ⇌ 2NO2(g)At a certain reaction conditions, the concentrations of NO, O2, and NO2 are 0.45 M, 0.25 M, and 0.60 M respectively. Determine if the reaction is at equilibrium and, if not, in which direction will it proceed to reach equilibrium.

asked Feb 3 in Chemical thermodynamics by ClairWaite7 (1.8k points)

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1 answer 121 views

Calculate the reaction quotient (Q) for the following chemical reaction at a given temperature and pressure: 2 SO2 (g) + O2 (g) ⟶ 2 SO3 (g) The initial concentrations of SO2, O2, and SO3 are 0.2 M, 0.1 M, and 0.3 M, respectively, at a total pressure of 3 atm and a temperature of 298 K.

asked Feb 3 in Chemical thermodynamics by StephaineCro (1.8k points)

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1 answer 127 views

Calculate the rate of the electrochemical reaction when a current of 2.5 A is passed through a solution of copper sulphate for 2 hours, and 4 g of copper is formed at the cathode. The atomic weight of copper is 63.5 g/mol.

asked Feb 3 in ElectroChemistry by ClevelandHaw (2.4k points)

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1 answer 93 views

Calculate the rate of the electrochemical reaction that takes place in the following electrolytic cell:Cu(s) | Cu2+(aq, 0.050 M) || Ag+(aq, 0.010 M) | Ag(s)Given that the current density is 0.500 A/m2 and the Faraday constant is 96,485 C/mol. The reduction potential of Cu2+(aq) + 2e- → Cu(s) is +0.34 V, and the reduction potential of Ag+(aq) + e- → Ag(s) is +0.80 V. Assume the temperature is 25°C and one-unit charge is exchanged.

asked Feb 3 in ElectroChemistry by FelixTolmer3 (1.9k points)

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1 answer 128 views

Calculate the rate of electroplating of copper on a metallic surface at a current of 2.5 amperes for a duration of 3 hours using a copper nitrate solution with a concentration of 0.2 M. Given that the standard potential of the reduction reaction of Cu2+ to Cu is +0.34 V and the charge of one mole of electrons is 96500 C/mol.

asked Feb 3 in ElectroChemistry by RudyMms5536 (1.8k points)

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1 answer 28 views

Calculate the rate constant at 300 K for a gas phase reaction with a rate of 0.025 M/s and an initial concentration of 0.10 M. The reaction is second order in the concentration of reactants.

asked Feb 3 in Physical Chemistry by RebekahH3016 (1.9k points)

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1 answer 143 views

Calculate the rate constant and the activation energy for the polymerization of styrene at 60°C, given that the rate of polymerization is 2.21 x 10^-3 mol L^-1 s^-1 at an initial concentration of 0.02 mol L^-1 and the activation energy is 101 kJ mol^-1.

asked Feb 3 in Polymer Chemistry by JudithMackni (2.3k points)

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1 answer 155 views

Calculate the quantity of heat required to melt 50.0 g of ice at its melting point (0°C). The enthalpy of fusion of water is 6.01 kJ/mol.

asked Feb 3 in ThermoChemistry by MiquelPlx868 (2.3k points)

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1 answer 126 views

Calculate the power output of an electrochemical cell that uses a cathode made of silver metal immersed in a solution containing silver ions with a concentration of 0.05 M and an anode made of zinc metal immersed in a solution containing zinc ions with a concentration of 0.1 M. The temperature of the solutions is 298 K and the cell operates at a current of 0.5 A.

asked Feb 3 in ElectroChemistry by EdytheEwk100 (2.6k points)

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1 answer 127 views

Calculate the power output of a galvanic cell having a standard potential of +0.76V and a current of 0.5A flowing through it. The cell consists of a zinc electrode and a copper electrode connected by a salt bridge and the concentration of the electrolyte is 1.0M. Given that the Faraday constant is 96487 C/mol and the temperature is 298K.

asked Feb 3 in ElectroChemistry by EvieOconnor (2.3k points)

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1 answer 97 views

Calculate the power output of a galvanic cell given that the cell potential is 1.8 V and the current passing through the circuit is 2.5 A. The electrochemical reaction taking place in the cell is the oxidation of Zinc and reduction of Copper. The standard reduction potentials are +0.76 V for copper and -0.76 V for zinc. The concentration of Zinc ions is 1.0 M whereas Copper ions concentration is 0.1 M. Determine the power output of the cell.

asked Feb 3 in ElectroChemistry by ElenaBriscoe (2.1k points)

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1 answer 128 views

Calculate the power output of a Galvanic cell consisting of a standard hydrogen electrode and a standard copper electrode at 298 K when the concentration of copper ions in the cathode half-cell is 0.1 M and hydrogen gas pressure in the anode half-cell is at 1 bar. The standard reduction potentials for the hydrogen and copper half-reactions are +0.0 V and +0.34 V, respectively.

asked Feb 3 in ElectroChemistry by VickeyBatema (1.9k points)

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1 answer 157 views

Calculate the power output for a Zinc-Copper electrochemical cell operating at standard conditions with a Zinc electrode that measures 10 cm by 12 cm and a Copper electrode that measures 8 cm by 10 cm. The current flowing through the circuit is 0.5 A. The standard reduction potentials for the half-reactions are +0.76 V for Cu2+/Cu and -0.76 V for Zn2+/Zn.

asked Feb 3 in ElectroChemistry by StarMayo945 (1.8k points)

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1 answer 144 views

Calculate the potential difference between two silver electrodes that are placed into a solution containing 0.1M of AgNO3 and a current of 2.5 A is passed through the cell. The polarization caused by the passage of current through the cell is found to be 0.2 V. Given that the standard reduction potential of Ag+ to Ag is 0.80 V, calculate the equilibrium potential of the cell.

asked Feb 3 in ElectroChemistry by CatherineMcc (2.5k points)

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1 answer 167 views

Calculate the polarization that occurs in an electrochemical cell when a current of 2 A flows through it for 10 minutes. The electrode area is 25 cm², and the current efficiency is 95%. The activation energy is 80 kJ/mol, and the reaction quotient is 2.5 x 10⁻⁵. The temperature of the cell is 25°C. Find the polarization resistance and the total polarization of the cell.

asked Feb 3 in ElectroChemistry by AleciaAlleyn (1.5k points)

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1 answer 119 views

Calculate the polarization resistance of a copper electrode in a 0.1 M copper sulfate solution at 25°C, given that the current density is 10 mA/cm² and the exchange current density is 0.1 mA/cm². The Tafel slope is 30 mV/decade.

asked Feb 3 in ElectroChemistry by HeidiElmslie (1.8k points)

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1 answer 195 views

Calculate the polarization potential in an electrochemical cell if the concentration of zinc ions in the anode compartment is 0.5 M, the concentration of copper(II) ions in the cathode compartment is 1.0 M, and the voltage of the cell is 1.1 V. The standard reduction potential of copper(II) ions is +0.34 V and the standard reduction potential of zinc ions is -0.76 V.

asked Feb 3 in ElectroChemistry by HesterLoyau3 (2.1k points)

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1 answer 140 views

Calculate the polarization of a copper-silver galvanic cell in which the concentration of copper ions is 0.5 M, the concentration of silver ions is 0.1 M, and the cell is operating at a temperature of 25°C. The potential difference of the cell is measured to be 0.75 V.

asked Feb 3 in ElectroChemistry by VioletteM27 (2.1k points)

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1 answer 91 views

Calculate the polarization of a copper electrode immersed in a 0.1 M CuSO4 solution at 25°C when it is coupled to a hydrogen electrode with a hydrogen pressure of 1 atm. Given that the standard reduction potential of Cu2+|Cu electrode is 0.34 V and the standard reduction potential of H+|H2 electrode is 0 V at 25°C.

asked Feb 3 in ElectroChemistry by JadaMeece33 (1.6k points)

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