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Considering the reaction: Zn(s) + Cu2+(aq) -> Cu(s) + Zn2+(aq) What is the cell potential (in volts) at 25°C when the concentrations of [Cu2+] and [Zn2+] are 0.5 M and 1.0 M, respectively, and the zinc electrode is the anode? The standard reduction potentials for Cu2+/Cu and Zn2+/Zn are 0.34 V and -0.76 V, respectively.

asked Feb 3 in ElectroChemistry by DexterTejada (1.7k points)

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What is the effect of changing the ligands on the photochemical properties of metal complexes? Provide specific examples and discuss the underlying mechanisms.

asked Feb 3 in PhotoChemistry by EdwinStambau (2.4k points)

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Calculate the standard electrode potential for the following reaction: Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)Given: Standard reduction potential for Ag+ + e- → Ag is 0.80 VStandard reduction potential for Cu2+ + 2e- → Cu is 0.34 V

asked Feb 3 in ElectroChemistry by 73351052550 (1.9k points)

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Calculate the standard enthalpy change for the sublimation of 5 moles of solid iodine (I2) given the following data:- Enthalpy of fusion of iodine = 15.52 kJ/mol- Enthalpy of vaporization of iodine = 41.57 kJ/mol

asked Feb 3 in Chemical thermodynamics by MaybellHoffm (2.2k points)

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How does changing the length of the hydrocarbon chain in a surfactant affect its ability to reduce surface tension?

asked Feb 3 in Surface Chemistry by JEAMolly3713 (2.3k points)

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How does changing the concentration of the reactants affect the rate of reaction and subsequently the profitability of the reaction?

asked Feb 3 in Chemical kinetics by JaysonPlott5 (1.6k points)

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Calculate the standard enthalpy change (∆H°) for the reaction: 2NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)Given the following bond dissociation energies (in kJ/mol):N≡N = 941, N-H = 391, O=O = 495, O-H = 464, N-O = 201, H-O-H = 464, N-H + O=O = 632, N=O = 607, and H-N≡N = 945.

asked Feb 3 in Quantum Chemistry by Phillipp57B1 (2.3k points)

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Calculate the standard enthalpy of formation of ammonia gas (NH3) using the following information:- Standard enthalpy of formation for nitrogen gas (N2) = 0 kJ/mol- Standard enthalpy of formation for hydrogen gas (H2) = 0 kJ/mol- Standard enthalpy of formation for ammonia gas (NH3) = -46 kJ/mol

asked Feb 3 in Chemical thermodynamics by JulianaKane (2.2k points)

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Calculate the standard cell potential of the following electrochemical cell: Ag(s) │ AgCl(s) │ Cl^-(aq, 0.040 M) ‖ Cu^2+(aq, 0.020 M) │ Cu(s) at 298 K. The reduction potential of AgCl/Ag couple is +0.22 V and the reduction potential of Cu^2+/Cu couple is +0.34 V.

asked Feb 3 in Physical Chemistry by XHQMikel9006 (2.0k points)

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Calculate the standard enthalpy change for the fusion of 1 mole of solid water (ice) at 0°C to liquid water at 0°C. Given the enthalpy of fusion of solid water as 6.01 kJ/mol and the specific heat capacity of water as 4.18 J/g°C.

asked Feb 3 in Chemical thermodynamics by BetteBoniwel (1.6k points)

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Calculate the standard cell potential of the following electrochemical cell at 298 K, given the half-reactions and their standard reduction potentials in brackets:Cu(s) | Cu^2+(0.001 M) || Ag+(0.1 M) | Ag(s)

asked Feb 3 in Physical Chemistry by GingerJ92570 (1.6k points)

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Calculate the standard enthalpy change for the reaction: CuSO4 (aq) + 4NH3 (aq) -> Cu(NH3)4SO4 (aq) given that the standard enthalpy changes of formation for CuSO4 (aq) and NH3 (aq) are -771.5 kJ/mol and -46.19 kJ/mol respectively, and the standard enthalpy change of formation for Cu(NH3)4SO4 (aq) is -2130.4 kJ/mol.

asked Feb 3 in Chemical thermodynamics by VickeyPeacoc (2.4k points)

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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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Consider the reaction: 2H2O (g) ⇄ 2H2 (g) + O2 (g) At 1000 K, the equilibrium constant Kc for this reaction is 4.17 x 10^-5. Suppose that initially, 0.10 moles of H2O, 0.20 moles of H2, and 0.20 moles of O2 are placed in a 1.0 L container at 1000 K. What will be the equilibrium concentrations of H2O, H2, and O2?

asked Feb 3 in Chemical equilibrium by MerryR11813 (1.7k points)

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Calculate the standard enthalpy change for the formation of ethylene glycol (C2H6O2) from its elements given that the standard enthalpies of formation of carbon dioxide, water, and ethylene glycol are -393.5 kJ/mol, -285.8 kJ/mol, and -421.1 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by ChiKellett4 (1.5k points)

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Calculate the standard enthalpy change (ΔH°) and standard entropy change (ΔS°) for the decomposition reaction of calcium carbonate (CaCO3) at 298 K:CaCO3(s) → CaO(s) + CO2(g)

asked Feb 3 in Inorganic Chemistry by MoniqueBrins (1.9k points)

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Calculate the standard enthalpy change for the reaction: [Co(H2O)6]2+(aq) + 4Cl-(aq) → [CoCl4]2-(aq) + 6H2O(l) Given the following information:• ΔH°f of [Co(H2O)6]2+ is 32.3 kJ/mol • ΔH°f of [CoCl4]2- is -341.8 kJ/mol • ΔH°f of H2O(l) is -285.8 kJ/mol • The ΔH°f of Cl- is taken as zero

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

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Calculate the standard enthalpy change for the formation of carbon dioxide (CO2) from its elements carbon (C) and oxygen (O2) given the following information:- The standard enthalpy change for the combustion of carbon to form carbon dioxide is -394 kJ/mol.- The standard enthalpy change for the combustion of hydrogen gas (H2) to form water (H2O) is -286 kJ/mol.- The standard enthalpy change for the reaction of oxygen gas (O2) with hydrogen gas (H2) to form water (H2O) is -572 kJ/mol.Note: All values are at standard temperature and pressure (298 K and 1 atm).

asked Feb 3 in Chemical thermodynamics by CandyDemaio (2.3k points)

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Calculate the standard free energy change for the following redox reaction at 298 K:Mg(s) + 2H+(aq) -> Mg2+(aq) + H2(g)Given: Eºred for Mg2+/Mg = -2.37 V & Eºred for H+/H2 = 0 V.

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

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Consider the following redox reaction:Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)Calculate the standard free energy change (ΔG°) for the reaction at 298K, given that the standard reduction potentials for Cu2+(aq)/Cu(s) and Ag+(aq)/Ag(s) are +0.34V and +0.80V, respectively.

asked Feb 3 in Chemical thermodynamics by WayneYcs587 (2.5k points)

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