Hot questions

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the following reaction:2Fe(s) + 3/2O2(g) → Fe2O3(s)Given that the standard enthalpy of formation of Fe2O3(s) is -824 kJ/mol and the standard enthalpy of formation of Fe(s) and O2(g) are 0 kJ/mol.

asked 4 days ago in Chemical thermodynamics by Kaley34M2669 (430 points)

0 votes

1 answer 33 views

Calculate the standard enthalpy change for the phase transition reaction from solid to liquid for a sample of substance X, given that the mass of the sample is 10 grams and the melting point of substance X is 50°C. The specific heat capacity of substance X is 2 J/g°C and the enthalpy of fusion for substance X is 50 J/g.

asked 4 days ago in Chemical thermodynamics by LizzieDechai (330 points)

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the following reaction: [Fe(H2O)6]2+(aq) + SO4 2-(aq) → [Fe(H2O)5 SO4]-(aq) + H2O(l) given that the standard enthalpies of formation of [Fe(H2O)6]2+, [Fe(H2O)5SO4]-, and H2O are -360 kJ/mol, -950 kJ/mol, and -286 kJ/mol, respectively.

asked 4 days ago in Chemical thermodynamics by BrendaBurche (450 points)

0 votes

1 answer 29 views

Calculate the volume of 0.2 M hydrochloric acid required to completely neutralize 25 mL of 0.1 M sodium hydroxide solution.

asked 4 days ago in Chemical reactions by Eduardo04095 (870 points)

0 votes

1 answer 32 views

Calculate the standard enthalpy change for the reaction of the combustion of 1 mole of liquid ethanol (C2H5OH) at 298K and 1 atm. The balanced chemical equation for the reaction is: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)Given:ΔHf°(C2H5OH(l)) = -277.7 kJ/molΔHf°(CO2(g)) = -393.5 kJ/molΔHf°(H2O(l)) = -285.8 kJ/molΔHf°(O2(g)) = 0 kJ/mol

asked 4 days ago in Chemical thermodynamics by VidaMcAlroy6 (470 points)

0 votes

1 answer 31 views

Calculate the standard enthalpy change of reduction for the reaction: Fe2O3(s) + 3H2(g) -> 2Fe(s) + 3H2O(l) Given: Standard enthalpy of formation (ΔHf°) of Fe2O3(s) = -822 kJ/mol Standard enthalpy of formation (ΔHf°) of H2O(l) = -286 kJ/mol Standard enthalpy of fusion (ΔHfus) of Fe(s) = 13.81 kJ/mol Standard enthalpy of vaporization (ΔHvap) of H2(g) = 0.449 kJ/mol Standard enthalpy of formation (ΔHf°) of H2(g) = 0 kJ/mol

asked 4 days ago in ThermoChemistry by QuinnSwank82 (410 points)

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the following reaction at 298 K:Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

asked 4 days ago in Quantum Chemistry by AlisonVinci (490 points)

0 votes

1 answer 32 views

Calculate the standard enthalpy change for the reaction of [Co(H2O)6]Cl2 and NaOH using the following balanced chemical equation and given standard enthalpies of formation:[Co(H2O)6]Cl2 (aq) + 2NaOH (aq) → [Co(H2O)6](OH)2 (s) + 2NaCl (aq)ΔH°f [Co(H2O)6]Cl2 (aq) = -415.32 kJ/molΔH°f [Co(H2O)6](OH)2 (s) = -1276.24 kJ/molΔH°f NaCl (aq) = -407.33 kJ/mol

asked 4 days ago in Chemical thermodynamics by AprilCutlack (610 points)

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the following reaction at 25°C given the enthalpies of formation (in kJ/mol) of the compounds involved:CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)Hf(CaCO3) = -1206.9 kJ/molHf(CaCl2) = -795.8 kJ/molHf(CO2) = -393.5 kJ/molHf(H2O) = -285.8 kJ/molHf(HCl) = -92.31 kJ/mol

asked 4 days ago in Chemical thermodynamics by JameHumphrie (670 points)

0 votes

1 answer 33 views

Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given that the reaction produces water and sodium chloride as products. The molar enthalpy of formation for water is -285.8 kJ/mol and for NaCl is -411.2 kJ/mol. The balanced chemical equation for the reaction is: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

asked 4 days ago in Chemical thermodynamics by PUPMora98542 (450 points)

0 votes

1 answer 30 views

Calculate the standard enthalpy of hydrolysis for the following reaction: AlCl3 + 3H2O → Al(OH)3 + 3HCl Given that the standard enthalpies of formation for AlCl3(-696.5 kJ/mol), Al(OH)3(-1277.1 kJ/mol), and HCl(-92.3 kJ/mol) are known.

asked 4 days ago in ThermoChemistry by JulioDarrow7 (750 points)

0 votes

1 answer 39 views

Calculate the specific heat capacity of water if it absorbs 400 J of energy and its temperature rises by 20°C.

asked 4 days ago in Chemical thermodynamics by PamalaDeNeev (490 points)

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the dissolution of 10 grams of NaCl in water at 25°C, given that the molar enthalpy of dissolution of NaCl is -3.9 kJ/mol.

asked 4 days ago in Chemical thermodynamics by JaniChewning (820 points)

0 votes

1 answer 33 views

Calculate the standard enthalpy change for the liquid-to-gas phase transition of water at 100°C and atmospheric pressure, given that the enthalpy of vaporization of water is 40.7 kJ/mol.

asked 4 days ago in Chemical thermodynamics by GeraldoMendi (370 points)

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the complete combustion of 2 moles of methane gas under standard conditions, where all reactants and products are in their standard states. The balanced chemical equation for the combustion of methane is CH4(g) + 2O2(g) → CO2(g) + 2H2O(l), and the standard enthalpy of formation ΔH°f for methane, carbon dioxide, and water are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.

asked 4 days ago in Chemical thermodynamics by YACCaryn271 (590 points)

0 votes

1 answer 26 views

Design a counter-current heat exchanger to cool 10,000 liters per hour of cyclohexane at 110°C down to 50°C, while heating 7,500 liters per hour of water at 25°C up to 80°C. The cyclohexane will be cooled by water which enters the heat exchanger at 90°C and exits at 60°C. The overall heat transfer coefficient is expected to be 1,000 W/m2K. Determine the required heat transfer area and the pressure drop across the heat exchanger.

asked 4 days ago in Chemical engineering by IleneNobles (190 points)

0 votes

1 answer 28 views

Consider a reaction where Ag is oxidized to Ag+ ions in a solution containing AgNO3. We set up an electrochemical cell with a Ag/Ag+ electrode as the anode and a platinum electrode as the cathode. The standard electrode potential for the Ag/Ag+ electrode is +0.80 V. What is the overpotential required to achieve a current of 2 A if the applied voltage is 1.00 V?

asked 4 days ago in ElectroChemistry by FatimaChatte (410 points)

0 votes

1 answer 29 views

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 4 days ago in ElectroChemistry by CarleyMcdono (410 points)

0 votes

1 answer 31 views

Calculate the standard enthalpy change for the reduction of iron (III) oxide using carbon monoxide as the reducing agent, given that the standard enthalpy of formation for iron (III) oxide is -824.2 kJ/mol and the standard enthalpy of formation for carbon monoxide is -110.5 kJ/mol.

asked 4 days ago in ThermoChemistry by PWOMazie102 (650 points)

0 votes

1 answer 37 views

Calculate the standard electrode potential (E°) for the redox reaction of the following half-reactions:Cu2+(aq) + 2e- → Cu(s) E° = +0.34 VFe3+(aq) + e- → Fe2+(aq) E° = +0.77 V

asked 4 days ago in Chemical thermodynamics by DawnAbraham (490 points)

Categories