Recent questions in ThermoChemistry

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Determine the standard enthalpy of formation for ammonium chloride (NH4Cl) using Hess's Law and the following given reactions: 1) N2(g) + 3H2(g) → 2NH3(g) ΔH° = -46.0 kJ/mol 2) NH3(g) + HCl(g) → NH4Cl(s) ΔH° = -176.2 kJ/mol 3) N2(g) + 2H2(g) + 2Cl2(g) → 2NH4Cl(s) ΔH° = -634.2 kJ/mol

asked Feb 4 in ThermoChemistry by ScottyWild8 (1.4k points)

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Determine the heat of hydration, in kJ/mol, for the reaction between solid Calcium chloride (CaCl2) and water (H2O), given that 1 mole of CaCl2 dissolves to produce 3 moles of ions and releases -82.8 kJ of heat in the process.

asked Feb 4 in ThermoChemistry by CherylDooley (1.7k points)

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1 answer 67 views

Determine the enthalpy of hydrolysis for sodium acetate (NaC2H3O2) given that the enthalpy of neutralization for acetic acid (HC2H3O2) and sodium hydroxide (NaOH) is -55.9 kJ/mol and the heat of formation for NaC2H3O2 is -382.7 kJ/mol.

asked Feb 4 in ThermoChemistry by EmilyUtley95 (1.9k points)

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Determine the enthalpy of desorption for carbon dioxide from activated charcoal at 25°C. Given: the equilibrium pressure of CO2 is 0.1 atm and the mass of charcoal used is 2.5 g.

asked Feb 4 in ThermoChemistry by JewelSchaffe (1.8k points)

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Determine the enthalpy of adsorption for the reaction of hydrogen gas adsorbing onto a platinum surface, given that 2.00 g of hydrogen gas is adsorbed onto a 1.00 g platinum surface at 25°C and the pressure is 1 bar. The volume of the system is 1.00 L and the initial temperature of the platinum surface is also 25°C. Assume that the surface is in thermal equilibrium with the surroundings and that the gas behaves ideally.

asked Feb 4 in ThermoChemistry by AlishaGuy35 (2.5k points)

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Determine the enthalpy change of precipitation for the reaction between 50ml of 0.1M sodium sulfate and 50ml of 0.1M barium nitrate, given that the final temperature is 25°C and the initial temperature was 30°C. The specific heat capacity of the solution is 4.18 J/g °C and the density is 1 g/mL. (Assume the reaction goes to completion and all volumes are additive.)

asked Feb 4 in ThermoChemistry by BFFRachelle (1.8k points)

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Determine the enthalpy change of precipitation for the reaction between 50 mL of 0.1 M NaOH and 50 mL of 0.1 M CuSO4, given that the final solution has a temperature of 25°C and the specific heat capacity of the solution is 4.18 J/g·°C.

asked Feb 4 in ThermoChemistry by LavernEcm901 (1.8k points)

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1 answer 82 views

Determine the enthalpy change for the oxidation of 2 moles of iron (Fe) to form iron oxide (FeO) using the following data: Fe + 1/2 O2 → FeO ΔH = -65.0 kJ/mol 4 Fe + 3 O2 → 2 Fe2O3 ΔH = -1648.6 kJ/mol

asked Feb 4 in ThermoChemistry by RenaCastella (1.7k points)

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Determine the bond dissociation energy of methane (CH4) using the following data: Reaction: CH4(g) → C(g) + 4H(g)ΔH°f (kJ/mol): CH4(g) = -74.81C(g) = 715.32H(g) = 218.00Hint: bond dissociation energy can be calculated using the formula ΔH°rxn = Σ (ΔH°f, products) - Σ (ΔH°f, reactants)

asked Feb 4 in ThermoChemistry by Bernice06378 (1.4k points)

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1 answer 40 views

Consider the following reactions:1. Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) ΔH₁ = -454.9 kJ/mol2. MgO(s) + 2HCl(aq) → MgCl₂(aq) + H₂O(l) ΔH₂ = -131.3 kJ/mol3. H₂(g) + ½O₂(g) → H₂O(l) ΔH₃ = -285.8 kJ/molUsing Hess's Law, calculate the enthalpy change for the following reaction:MgO(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) given that the enthalpy change for the reaction Mg(s) + ½O₂(g) → MgO(s) is ΔH = -601.6 kJ/mol.

asked Feb 3 in ThermoChemistry by AdaFennescey (1.8k points)

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1 answer 79 views

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 ChasityLearm (2.1k points)

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1 answer 84 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 MargueriteSa (2.1k points)

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1 answer 42 views

Calculate the standard enthalpy of reduction for the following reaction: Fe2O3 (s) + 3 H2(g) → 2 Fe(s) + 3 H2O(g)Given: ΔH°f for Fe2O3 (s) = -824.2 kJ/mol ΔH°f for H2O(g) = -241.8 kJ/molΔH°f for Fe(s) = 0 kJ/mol

asked Feb 3 in ThermoChemistry by PeteWirtz263 (2.1k points)

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1 answer 56 views

Calculate the standard enthalpy of precipitation for the reaction: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) given that the standard enthalpies of formation for AgNO3(aq), NaCl(aq), AgCl(s), and NaNO3(aq) are -123.2 kJ/mol, -407.3 kJ/mol, -127.0 kJ/mol, and -467.3 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by NickolasShum (1.9k points)

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1 answer 101 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 Feb 3 in ThermoChemistry by DelilahKyte3 (1.8k points)

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1 answer 67 views

Calculate the standard enthalpy of hydrolysis for Na2CO3 when 2.5 moles of water react with 1 mole of Na2CO3, given that the heat of reaction is -843.2 kJ/mol.

asked Feb 3 in ThermoChemistry by LillianaY16 (1.7k points)

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Calculate the standard enthalpy of formation, ΔH°f, of carbon dioxide (CO2) gas given the following thermochemical equations: C(s) + O2(g) → CO2(g) ΔH°rxn = -393.5 kJ/mol C(s) + O2(g) → CO(g) ΔH°rxn = -110.5 kJ/mol CO(g) + 1/2 O2(g) → CO2(g) ΔH°rxn = -283.0 kJ/mol Assume that all reactants and products are in their standard states.

asked Feb 3 in ThermoChemistry by Karine04K24 (2.0k points)

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1 answer 63 views

Calculate the standard enthalpy of formation of water (H2O) given the following information:- The standard enthalpy of formation of hydrogen gas (H2) is 0 kJ/mol- The standard enthalpy of formation of oxygen gas (O2) is 0 kJ/mol- The standard enthalpy of combustion of hydrogen gas is -286 kJ/mol- The standard enthalpy of combustion of carbon (C) is -394 kJ/mol- The standard enthalpy of combustion of methane gas (CH4) is -890 kJ/mol

asked Feb 3 in ThermoChemistry by ChiKellett4 (1.5k points)

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1 answer 46 views

Calculate the standard enthalpy of formation of water (H2O) given the following information: ΔHf° of H2(g) = 0 kJ/molΔHf° of O2(g) = 0 kJ/molΔHf° of H2O2(l) = -188.2 kJ/mol

asked Feb 3 in ThermoChemistry by Lavonda96B02 (2.3k points)

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1 answer 67 views

Calculate the standard enthalpy of formation of methanol, CH3OH (l), given that the standard enthalpy of combustion of methanol is -726.4 kJ/mol and the standard enthalpy of formation of carbon dioxide and water are -393.5 kJ/mol and -285.8 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by Miguel37A006 (2.3k points)

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