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Calculate the reaction quotient, Qc, for the following reaction:2NO2(g) + 7H2(g) → 2NH3(g) + 4H2O(g)at a temperature of 300 K and a pressure of 0.5 atm for each gas species. The equilibrium constants, Kc, at the same temperature and pressure are:Kc = 0.0080 for the reverse reactionKc = 7.2 × 10^-7 for the forward reaction

asked Feb 3 in Chemical thermodynamics by SvenMcConnel (1.3k points)

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1 answer 76 views

Calculate the reaction quotient, Q, for the following reaction at room temperature:$$\ce{CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g)}$$Given:- Partial pressure of methane, $\ce{CH4}$ = 0.25 atm- Partial pressure of oxygen, $\ce{O2}$ = 0.75 atm- Partial pressure of carbon dioxide, $\ce{CO2}$ = 0.0 atm- Partial pressure of water vapor, $\ce{H2O(g)}$ = 0.0 atmUse Q to determine if the reaction is at equilibrium, or if it will shift towards the products or reactants to reach equilibrium.

asked Feb 3 in Chemical thermodynamics by BarrettGriff (2.0k points)

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1 answer 66 views

Calculate the reaction quotient, Q, for the following balanced chemical reaction at 298 K:2NO(g) + O2(g) ⇌ 2NO2(g)Given that the initial concentrations of NO, O2 and NO2 are 0.10 M, 0.15 M and 0.05 M, respectively.

asked Feb 3 in Chemical thermodynamics by LidiaBautist (1.4k points)

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1 answer 37 views

Calculate the reaction quotient Q for the chemical reaction below using the given concentrations of reactants and products at a temperature of 25°C:2H2(g) + O2(g) -> 2H2O(g)[H2] = 0.10 M, [O2] = 0.05 M, [H2O] = 0.08 M.

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

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1 answer 68 views

Calculate the reaction quotient (Qc) for the following reaction at 298 K and 1 atm: 2 NO2(g) + F2(g) ⇌ 2 NO2F(g)Given the molar concentrations of reactants and products are [NO2] = 0.25 M, [F2] = 0.15 M, and [NO2F] = 0.10 M at equilibrium.

asked Feb 3 in Chemical thermodynamics by JulianKnetes (2.0k points)

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1 answer 45 views

Calculate the reaction quotient (Qc) for the following reaction at 25°C, given the concentration of reactants and products:2NO2(g) + F2(g) ⇌ 2NO2F(g)[NO2] = 0.30 M, [F2] = 0.40 M, [NO2F] = 0.60 M.Is the reaction at equilibrium? If not, in which direction will the reaction proceed to achieve equilibrium?

asked Feb 3 in Chemical thermodynamics by LizaSwenson (1.7k points)

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1 answer 54 views

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 63 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 60 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 64 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 50 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 57 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 15 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 77 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 81 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 59 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 60 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 52 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 39 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 91 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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