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A beaker of water is placed on a hot plate, and the temperature is gradually increased. Write an equation for the rate of change of entropy with respect to time during this process, assuming the system is not in equilibrium. Use the equation to determine the rate of entropy production in the water as it is heated from 25°C to 100°C at a constant rate of 2°C/min.

asked Jan 22 in Physical Chemistry by RobertoMundy (1.7k points)

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1 answer 78 views

Calculate the bond dissociation energy (in kJ/mol) of the H-Cl bond in hydrogen chloride molecule, given that the bond length is 127 pm and the vibrational frequency is 8.8 x 10^13 Hz.

asked Jan 23 in Chemical bonding by ThadGoetz093 (1.6k points)

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1 answer 63 views

Calculate the exchange current density for a Zinc electrode immersed in a solution containing 0.1 M Zinc ions at 25 degrees Celsius, given that the standard potential of the Zinc half-reaction is -0.76 V and the transfer coefficient is 0.5. (Assume concentration polarization effects to be negligible.)

asked Jan 23 in ElectroChemistry by KassieStarns (2.3k points)

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1 answer 80 views

Calculate the amount of copper deposited on the cathode when a current of 5 amperes is passed through a copper sulfate solution for a duration of 30 minutes. The molar mass of copper is 63.55 g/mol and the Faraday constant is 96500 C/mol. The electrode area is 10 cm² and the copper sulfate solution has a concentration of 0.1 M. Assume 100% efficiency in the electrochemical reaction.

asked Jan 23 in ElectroChemistry by ChristianeBo (2.0k points)

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1 answer 64 views

Calculate the entropy change (∆S) for the reaction between 2.0 moles of hydrogen gas (H2) and 1.0 mole of oxygen gas (O2) at constant pressure and a temperature of 298 K, given the standard molar entropy values for H2 and O2 to be 130.7 J/K•mol and 205.0 J/K•mol, respectively.

asked Jan 23 in ThermoChemistry by RoderickKyle (2.4k points)

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1 answer 71 views

Calculate the enthalpy change of ionization for hydrogen gas when one mole of H2 gas is ionized to form two moles of H+ ions in the gas phase, given that the enthalpy change of ionization for H(g) is +1312 kJ/mol.

asked Jan 23 in ThermoChemistry by OnaSchnell25 (1.8k points)

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1 answer 80 views

Calculate the activation energy for a chemical reaction that has a rate constant of 0.007 mol/L/s at 25°C and 0.059 mol/L/s at 35°C.

asked Jan 23 in Chemical reactions by CheryleKirso (2.1k points)

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1 answer 76 views

Calculate the concentration of Cu2+ ions in a 0.1 M CuSO4 solution using the given standard reduction potential of Cu2+/Cu electrode and the measured cell potential. The electrode potential of the cell is 0.78 V and temperature is 25°C.

asked Jan 23 in ElectroChemistry by DemetriusCha (1.7k points)

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1 answer 116 views

A chemistry student needs to determine the effect of adding NaCl to a solution containing AgNO3 at equilibrium. The original solution had concentration [Ag+]=0.01M and [NO3-]=0.01M, and Ksp=1.8x10^-10. How much NaCl (in grams) is needed to be added to the solution in order to decrease the [Ag+] concentration by a factor of 10?

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

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1 answer 68 views

Calculate the enthalpy of isomerization for butene to isobutene given the following bond dissociation energies (in kJ/mol): C-C = 345, C=C = 614, C-H = 413.

asked Jan 23 in ThermoChemistry by TraceeKeith9 (1.8k points)

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1 answer 117 views

A chemistry student is given an unknown compound and asked to identify it using mass spectrometry. The mass spectrum of the compound shows a molecular ion peak at m/z 150, a base peak at m/z 135, and a few smaller peaks at m/z 91, 77, and 65. What is the possible molecular formula of the unknown compound?

asked Jan 22 in Analytical Chemistry by Lavonda96B02 (2.3k points)

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1 answer 76 views

Calculate the change in entropy and enthalpy for the reaction of iron (III) oxide with carbon monoxide to form iron and carbon dioxide, given the following information:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)ΔH°f (Fe2O3) = -824.2 kJ/molΔH°f (CO) = -110.5 kJ/molΔH°f (Fe) = 0 kJ/molΔH°f (CO2) = -393.5 kJ/molΔS° (Fe2O3) = 87.4 J/K molΔS° (CO) = 197.9 J/K molΔS° (Fe) = 27.3 J/K molΔS° (CO2) = 213.6 J/K mol

asked Jan 23 in Inorganic Chemistry by ShadArchie3 (1.7k points)

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1 answer 317 views

What is the difference between instrumental and expressive leadership?

asked Jan 17 in Psychology by TonyaCombs22 (1.8k points)

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1 answer 62 views

Calculate the Gibbs free energy change (ΔG) for the reaction:N2(g) + 3H2(g) ⇌ 2NH3(g)Given the standard Gibbs free energy of formation (ΔG°f) values at 298 K are:ΔG°f of NH3(g) = -16.6 kJ/molΔG°f of N2(g) = 0 kJ/molΔG°f of H2(g) = 0 kJ/molAssume ideal gas behavior for all gases involved in the reaction.

asked Jan 23 in Chemical thermodynamics by HiramFarrell (1.7k points)

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1 answer 70 views

Calculate the enthalpy change when solid sodium hydroxide (NaOH) is dissolved into water, given that the desorption enthalpy of NaOH is 44.51 kJ/mol and the molar heat of solution is -44.51 kJ/mol.

asked Jan 23 in ThermoChemistry by LeesaJ55672 (1.9k points)

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1 answer 72 views

Calculate the enthalpy change for the following reaction using Hess's Law calculations:2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)Given the following information:2H2(g) + O2(g) → 2H2O(l) ΔH1 = -484 kJ/mol2S(s) + 3O2(g) → 2SO3(g) ΔH2 = -791 kJ/mol2H2(g) + S(s) → 2H2S(g) ΔH3 = -36 kJ/mol

asked Jan 23 in ThermoChemistry by DanialCheste (1.6k points)

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1 answer 77 views

Calculate the bond energy required to break a single bond between two nitrogen atoms in a molecule of nitrogen gas (N2), given that the bond dissociation energy of N2 is 945 kJ/mol.

asked Jan 23 in Chemical reactions by HungObryan8 (2.4k points)

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1 answer 61 views

Calculate the heat of formation of Methane (CH4), given the following enthalpy changes:- Enthalpy change of combustion of methane = -890.4 kJ mol^-1- Enthalpy change of formation of water = -285.8 kJ mol^-1- Enthalpy change of formation of carbon dioxide = -393.5 kJ mol^-1

asked Jan 23 in Chemical bonding by ClydeC545764 (2.2k points)

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1 answer 68 views

Calculate the enthalpy of formation of carbon dioxide given the following data:C(s) + O2(g) → CO2(g) ΔH° = -393.5 kJ/molC(s) + 2H2(g) → CH4(g) ΔH° = -74.8 kJ/mol2H2(g) + O2(g) → 2H2O(l) ΔH° = -571.6 kJ/mol

asked Jan 23 in ThermoChemistry by IsabelleTitu (1.8k points)

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1 answer 71 views

Calculate the enthalpy change for the reaction of burning 1 mole of methane using Hess's Law, given the following information:1) Enthalpy of formation for methane = -74.8 kJ/mol2) Enthalpy of combustion for methane = -890.3 kJ/mol3) Enthalpy of formation for water = -285.8 kJ/mol4) Enthalpy of formation for carbon dioxide = -393.5 kJ/mol

asked Jan 23 in ThermoChemistry by HiramFarrell (1.7k points)

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