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Calculate the standard enthalpy change for the neutralization of 50 mL of 0.1 M hydrochloric acid with 50 mL of 0.1 M sodium hydroxide at a constant temperature of 25°C, given that the specific heat capacity of the resulting solution is 4.18 J/g°C and its density is 1 g/mL.

asked Feb 3 in Chemical thermodynamics by DwayneBoatma (510 points)

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What is the effect of changing the concentration of reactants on the reaction rate and yield of a chemical reaction?

asked Feb 3 in Chemical kinetics by CecilB463053 (310 points)

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How does changing the temperature affect the equilibrium constant (Kc) and the formation of Fe(SCN)2+ complex ion from Fe3+ and SCN- ions?

asked Feb 3 in Chemical equilibrium by ElsaLoman15 (350 points)

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Calculate the standard enthalpy change for the vaporization of 1 mole of water at 100°C, given that the enthalpy of fusion of water is 6.01 kJ/mol and the enthalpy of vaporization of water is 40.7 kJ/mol.

asked Feb 3 in Chemical thermodynamics by RyanTom37685 (570 points)

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Calculate the resistance of a electrochemical cell at 25°C if the standard reduction potential of the anode is -1.36 V and the standard reduction potential of the cathode is +0.40 V. The solution contains 0.1 M CuSO4 and 0.01 M ZnSO4. The distance between the two electrodes is 5 cm and the cross-sectional area of each electrode is 2.5 cm².

asked Feb 3 in ElectroChemistry by VictorOdom61 (410 points)

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How does changing the surface ligands of gold nanoparticles affect their stability and reactivity in aqueous solution, as analyzed through molecular dynamics simulations?

asked Feb 3 in Computational Chemistry by FrankieBerge (270 points)

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Calculate the standard enthalpy change for the combustion of methane gas at standard conditions, given the following balanced chemical equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)Note: Standard conditions refer to a temperature of 25°C and a pressure of 1 atm.

asked Feb 3 in Chemical thermodynamics by GerardMaes99 (410 points)

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How does changing the surface chemistry of a solid surface affect the adsorption of proteins, and how can this knowledge be applied to improve biomaterials design for medical implants?

asked Feb 3 in Surface Chemistry by DebraAtkinso (230 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 SerenaMarcha (310 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 AudraKinard1 (390 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 AurelioSting (350 points)

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Calculate the standard enthalpy of formation for propene (C3H6) given that the standard enthalpy of combustion of propene is -1411.1 kJ/mol and the standard enthalpy of formation of carbon dioxide (CO2) and water (H2O) are -393.5 kJ/mol and -285.8 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by LeoraBoulton (290 points)

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1 answer 26 views

Calculate the standard enthalpy change for the precipitation reaction of solid silver chloride (AgCl) from the aqueous solution with the precipitation agent, hydrochloric acid (HCl). Given the molar enthalpies of formation of AgCl(s) and HCl(g) are -127.01 kJ/mol and -92.31 kJ/mol, respectively. The balanced equation for the reaction is: AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)

asked Feb 3 in Chemical thermodynamics by AHBJim662535 (610 points)

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

asked Feb 3 in Chemical kinetics by TresaMebane7 (410 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 ConstanceScr (430 points)

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1 answer 23 views

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 DesireeNaqui (370 points)

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1 answer 26 views

Calculate the standard enthalpy change for the phase transition reaction of ice to water at a constant pressure of 1 atm, given the following information:- The standard enthalpy of fusion for ice is 6.01 kJ/mol.- The molar heat capacity of ice is 36.8 J/(mol K).- The molar heat capacity of liquid water is 75.3 J/(mol K).- The melting point of ice is 0°C.- The boiling point of water is 100°C.

asked Feb 3 in Chemical thermodynamics by SanfordRobso (710 points)

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1 answer 23 views

Calculate the standard free energy change (∆G°) for the reaction: 2CH4(g) + 3O2(g) → 2CO2(g) + 2H2O(l) at 298 K, given that the standard enthalpy change (∆H°) of the reaction is -890.4 kJ mol^-1 and the standard entropy change (∆S°) of the reaction is +292.2 J K^-1 mol^-1. Is the reaction spontaneous or non-spontaneous under standard conditions?

asked Feb 3 in Physical Chemistry by ArlenAbt9111 (530 points)

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1 answer 24 views

Calculate the standard enthalpy change of the dissolution reaction for 5.00 g of NaOH in 100 mL of water, given the molar heat of solution of NaOH as -44.5 kJ/mol.

asked Feb 3 in Chemical thermodynamics by MarilouTafoy (630 points)

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Calculate the standard enthalpy change of reduction for the following reaction: Cu2+(aq) + 2e- -> Cu(s) Given that the standard electrode potential of Cu2+(aq)/Cu(s) is +0.34 V and the standard electrode potential of Ag+(aq)/Ag(s) is +0.80 V.

asked Feb 3 in ThermoChemistry by CorinneMcwho (470 points)

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