Recent questions in Chemistry

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Calculate the value of standard enthalpy change for the sublimation of solid iodine at 25°C. The molar heat capacity of iodine (s) is 54.44 J/mol·K and its molar entropy of sublimation is 62.43 J/mol·K. The standard entropy of formation of iodine (s) is 62.80 J/mol·K.

asked Feb 3 in Chemical thermodynamics by RussellOdoms (190 points)

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Calculate the total resistance of an electrochemical cell consisting of two half-cells where one half-cell has a copper electrode submerged in a 0.5 M CuSO4 solution, and the other half-cell has a zinc electrode submerged in a 1.0 M ZnSO4 solution. The copper electrode is connected to the zinc electrode through a salt bridge. The resistance of the salt bridge is 22 ohms, and the resistance of the copper and zinc electrodes are negligible.

asked Feb 3 in ElectroChemistry by Junko57E850 (270 points)

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Calculate the total heat change when 100 ml of 0.5 M HCl is mixed with 100 ml of 0.5 M NaOH at 25°C. Assume the heat capacity of the solution is 4.18 J/(g°C) and the density of the solution is 1 g/mL. The enthalpy of neutralization of HCl and NaOH is -57.3 kJ/mol.

asked Feb 3 in ThermoChemistry by TwilaColby85 (330 points)

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Calculate the theoretical yield of benzocaine that can be produced from 1.5 moles of p-aminobenzoic acid and excess ethanol, assuming complete conversion and a 95% yield.

asked Feb 3 in Chemical synthesis by DannySantora (390 points)

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1 answer 41 views

Calculate the surface tension of water at a temperature of 25°C using the capillary rise method, given that the diameter of the capillary tube is 0.8 mm and the rise of water in the tube is 3 cm.

asked Feb 3 in Surface Chemistry by FawnContrera (340 points)

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Calculate the surface tension of a liquid whose weight is 0.1 N and the length of a wire that floats on the surface of the liquid is 20 cm. The density of the liquid is 1.2 g/cm³.

asked Feb 3 in Surface Chemistry by ZackFarrell1 (250 points)

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Calculate the surface area of a solid adsorbent material using BET theory, given that the mass of the adsorbent material is 2.5 g, the area occupied by each adsorbed layer is 15 Å², the number of monolayers formed is 4, and the value of the BET constant is 0.05.

asked Feb 3 in Surface Chemistry by Alva13091412 (310 points)

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Calculate the standard reaction entropy of the reaction: 2Fe(s) + 3/2O2(g) --> Fe2O3(s) given that the standard enthalpy of the reaction is -824.2 kJ/mol at 298K.

asked Feb 3 in Inorganic Chemistry by RuebenBarnes (550 points)

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1 answer 46 views

Calculate the standard potential of the cell Ag(s) | Ag+(aq, 0.0100 M) || Cu2+(aq, 1.00 M) | Cu(s) at 25°C.

asked Feb 3 in ElectroChemistry by MarisaReeder (270 points)

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Calculate the standard potential of a Daniell cell if the concentration of copper ions and zinc ions in their respective half-cells is 1.0 M and the temperature of the cell is 25°C. The standard reduction potentials of copper and zinc electrodes are +0.34 V and -0.76 V respectively.

asked Feb 3 in Physical Chemistry by Otto41M9339 (270 points)

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Calculate the standard molar entropy change for the reaction: 2 SO2(g) + O2(g) → 2 SO3(g) at 298 K, given the following standard molar entropies: ΔS°(SO2(g)) = 248.2 J K^-1 mol^-1 ΔS°(O2(g)) = 205.0 J K^-1 mol^-1 ΔS°(SO3(g)) = 256.2 J K^-1 mol^-1

asked Feb 3 in Quantum Chemistry by ConnorWatkin (330 points)

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1 answer 49 views

Calculate the standard molar entropy change (∆S°) at 298 K for the reaction: 2H2 (g) + O2 (g) → 2H2O (l) given that the standard molar enthalpy change (∆H°) for this reaction is -572 kJ/mol.

asked Feb 3 in Quantum Chemistry by WilburPeters (490 points)

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Calculate the standard molar enthalpy change for the following reaction using quantum chemistry and compare it with the literature value: 2H2(g) + O2(g) -> 2H2O(g) Literature Value: -572 kJ/mol

asked Feb 3 in Quantum Chemistry by HalinaIvy91 (310 points)

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1 answer 58 views

Calculate the standard heat of mixing when 50 mL of 1 M HCl is mixed with 100 mL of 1 M NaOH at 25°C. The standard heat of neutralization of 1 M HCl and 1 M NaOH is -57.32 kJ/mol.

asked Feb 3 in ThermoChemistry by AlisaCamidge (270 points)

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1 answer 40 views

Calculate the standard heat of formation of water (H2O) using the bond dissociation energies of H2 and O2 and the standard heat of combustion of methane (CH4).

asked Feb 3 in Chemical bonding by JessieStraub (190 points)

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1 answer 58 views

Calculate the standard heat of formation (in kJ/mol) of water (H2O) given the following bond energies: H-H = 436 kJ/mol, O=O = 498 kJ/mol, H-O = 463 kJ/mol.

asked Feb 3 in Chemical bonding by ReganPennell (510 points)

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1 answer 40 views

Calculate the standard Gibbs free energy change, ΔG°, for the electrochemical reaction of 2 moles of aluminum (Al) being oxidized to form 3 moles of aluminum oxide (Al2O3) in a standard state. Given that E°cell for the reaction is 1.66 V and the standard potential for the reduction of Al3+ ions to Al is -1.66 V.

asked Feb 3 in ElectroChemistry by SusanClaborn (290 points)

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1 answer 57 views

Calculate the standard Gibbs free energy change for the reaction that occurs when a cell consisting of a nickel electrode and a silver electrode is connected, given that the nickel electrode is immersed in a solution containing 0.010 M Ni2+ ions and the silver electrode is immersed in a solution containing 0.20 M Ag+ ions. The standard reduction potential for the Ni2+/Ni half-cell is -0.25 V and for the Ag+/Ag half-cell is +0.80 V.

asked Feb 3 in ElectroChemistry by LyndaGrevill (190 points)

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Calculate the standard Gibbs free energy change for the following electrochemical reaction at 25°C:Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s) Given: E°cell = 0.46 V, F = 96,500 C/mol, R = 8.314 J/K·mol, and the standard reduction potentials at 25°C are Cu²⁺(aq) + 2e⁻ → Cu(s) (E°red = 0.34 V) and Ag⁺(aq) + e⁻ → Ag(s) (E°red = 0.80 V).

asked Feb 3 in ElectroChemistry by Victor294844 (370 points)

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1 answer 55 views

Calculate the standard Gibbs free energy change for the following chemical reaction at 25°C:2H2(g) + O2(g) → 2H2O(l)The standard Gibbs free energy of formation at 25°C for H2O(l) is -237.2 kJ/mol, H2(g) is 0 kJ/mol, and O2(g) is 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by ChetChadwick (250 points)

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