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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 standard enthalpy of formation for acetic acid (CH3COOH) using Hess's law and the following thermochemical equations:1) C(s) + O2(g) → CO2(g) ΔH = -394 kJ/mol2) 2H2(g) + O2(g) → 2H2O(l) ΔH = -572 kJ/mol3) C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH = -1234 kJ/mol4) CH3COOH(l) + O2(g) → CO2(g) + H2O(l) ΔH = ?

asked Feb 4 in Chemical thermodynamics by WillieAlgera (1.5k points)

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1 answer 81 views

Determine the standard enthalpy change of the reaction between 50.0 mL of 0.200 M hydrochloric acid (HCl) and 50.0 mL of 0.100 M sodium hydroxide (NaOH) at 25°C. The reaction is a neutralization reaction between HCl and NaOH, and the products are water and sodium chloride (NaCl). The molar enthalpy of formation of NaCl is -411.2 kJ/mol, and the specific heat capacity of the aqueous solution is 4.18 J/g°C.

asked Feb 4 in Chemical thermodynamics by ChristieJzq (1.7k points)

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1 answer 49 views

Determine the standard enthalpy change of the precipitation reaction between aqueous solutions of copper (II) sulfate and calcium hydroxide, given that the reaction produces copper (II) hydroxide, solid calcium sulfate and water as the products. The initial concentrations of the solutions are 0.1 M for copper (II) sulfate and 0.05 M for calcium hydroxide, and the reaction takes place at constant pressure and temperature of 25°C.

asked Feb 4 in Chemical thermodynamics by YvetteLink0 (2.0k points)

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Determine the standard enthalpy change of the dissolution reaction of 2.50 g of NaOH in water, given that the molar enthalpy of hydration of Na+ and OH- ions are -406.8 kJ/mol and -230.0 kJ/mol respectively. The heat capacity of the calorimeter is 25.2 J/°C and the initial and final temperatures were 24.0°C and 29.2°C respectively.

asked Feb 4 in Chemical thermodynamics by AustinL82055 (1.8k points)

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1 answer 58 views

Determine the standard enthalpy change for the vaporization of 50g of ethyl alcohol (C2H5OH) at its normal boiling point of 78.4°C. Given that the molar heat of vaporization of ethyl alcohol is 38.56 kJ/mol and the molar mass of ethyl alcohol is 46.07 g/mol.

asked Feb 4 in Chemical thermodynamics by KaitlynRodri (2.0k points)

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1 answer 78 views

Determine the standard enthalpy change for the reaction: Fe2O3 (s) + 3CO (g) → 2Fe (s) + 3CO2 (g)given the following values of standard enthalpy of formation:ΔHf° [Fe2O3 (s)] = -824 kJ/mol ΔHf° [CO2 (g)] = -393.5 kJ/mol ΔHf° [CO (g)] = -110.5 kJ/mol ΔHf° [Fe (s)] = 0 kJ/mol

asked Feb 4 in Chemical thermodynamics by MatthewStore (1.3k points)

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1 answer 61 views

Determine the standard enthalpy change for the reaction between calcium oxide and hydrochloric acid, given the following information:CaO(s) + 2HCl(aq) → CaCl2(aq) + H2O(l)∆Hf° CaCl2(aq) = -795.7 kJ/mol∆Hf° H2O(l) = -285.8 kJ/mol∆Hc° = -1922.6 kJ/mol

asked Feb 4 in Chemical thermodynamics by CarmellaBibl (2.0k points)

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1 answer 74 views

Determine the standard enthalpy change for the precipitation reaction of 10.0 g of calcium chloride (CaCl2) with excess sodium carbonate (Na2CO3) to form calcium carbonate (CaCO3) and sodium chloride (NaCl). Given the following standard enthalpies of formation: ΔHf°(CaCl2) = -795.8 kJ/mol, ΔHf°(Na2CO3) = -1130.1 kJ/mol, ΔHf°(CaCO3) = -1206.9 kJ/mol, and ΔHf°(NaCl) = -411.2 kJ/mol.

asked Feb 4 in Chemical thermodynamics by IDQMyles1187 (2.5k points)

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1 answer 67 views

Determine the standard enthalpy change for the precipitation reaction between aqueous solutions of silver nitrate (AgNO3) and potassium chloride (KCl), given the molar concentrations of AgNO3 and KCl are 0.10 M and 0.20 M, respectively. The balanced chemical equation for the reaction is:AgNO3(aq) + KCl(aq) -> AgCl(s) + KNO3(aq)The enthalpies of formation for AgNO3(aq), KCl(aq), AgCl(s), and KNO3(aq) are -365.6 kJ/mol, -436.0 kJ/mol, -127.0 kJ/mol, and -494.6 kJ/mol, respectively.

asked Feb 4 in Chemical thermodynamics by CorneliusMen (2.2k points)

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1 answer 74 views

Determine the standard enthalpy change for the formation of water (H2O) when hydrogen gas (H2) reacts with oxygen gas (O2) according to the balanced equation:2H2(g) + O2(g) → 2H2O(l)Given that the standard enthalpy change of formation for H2O(l) is -285.8 kJ/mol, calculate the amount of heat absorbed or released when 4.50 moles of H2O(l) is formed under standard conditions.

asked Feb 4 in Chemical thermodynamics by CIGArmando01 (1.8k points)

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1 answer 76 views

Determine the standard enthalpy change for the formation of methane gas (CH4) from its constituent elements (C and H2) given the following standard enthalpy of formation values: ΔHf°(C) = 0 kJ/mol and ΔHf°(H2) = 0 kJ/mol.

asked Feb 4 in Chemical thermodynamics by MargotFalkin (2.1k points)

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1 answer 59 views

Determine the standard enthalpy change for the following reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) Given:ΔHf°[Fe2O3(s)] = -824.2 kJ/mol ΔHf°[CO(g)] = -110.5 kJ/mol ΔHf°[Fe(s)] = 0 kJ/mol ΔHf°[CO2(g)] = -393.5 kJ/mol

asked Feb 4 in Chemical thermodynamics by ClaraCraddoc (1.6k points)

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1 answer 32 views

Determine the standard enthalpy change for the following reaction: 2 Fe (s) + 3/2 O2 (g) → Fe2O3 (s) Given the following data: - ΔHf° of Fe2O3 (s) = -826 kJ/mol - ΔHf° of O2 (g) = 0 kJ/mol - The heat capacity of the calorimeter is 135 J/°C Assume that the reaction takes place at constant pressure and that the heat absorbed by the calorimeter is negligible.

asked Feb 4 in Chemical thermodynamics by EttaKee54894 (2.1k points)

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1 answer 57 views

Determine the standard enthalpy change for the dissolution of 5.00 grams of magnesium chloride in water, given that the molar mass of MgCl2 is 95.21 g/mol and the standard enthalpy change of formation for magnesium chloride is -641.3 kJ/mol.

asked Feb 4 in Chemical thermodynamics by EdithLindt35 (1.6k points)

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1 answer 63 views

Determine the standard electrode potential, given that the standard reduction potential for the half-reaction, Ag+ (aq) + e- → Ag(s) is +0.80 V and the standard oxidation potential for the half-reaction, Fe(s) → Fe2+(aq) + 2e-, is -0.44 V. Using this information, predict whether or not the reaction Ag(s) + Fe2+(aq) → Fe(s) + Ag+(aq) will occur spontaneously under standard conditions.

asked Feb 4 in Chemical thermodynamics by Miguel37A006 (2.3k points)

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1 answer 57 views

Determine the rate law for the reaction of nitrogen dioxide with hydrogen gas, if the reaction rate is directly proportional to the concentration of nitrogen dioxide and the square of the concentration of hydrogen gas. Express the rate law in terms of the rate constant and the concentrations of the reactants.

asked Feb 4 in Chemical kinetics by BeverlyNavar (1.8k points)

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1 answer 72 views

Determine the possible isomers of C3H8O using structural formulas and name the type of isomerism for each.

asked Feb 4 in Chemical bonding by ChristelZ81 (1.7k points)

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1 answer 67 views

Determine the polarity of the H-Cl bond in hydrogen chloride molecule, given the electronegativity values of hydrogen and chlorine to be 2.2 and 3.0, respectively.

asked Feb 4 in Chemical bonding by JedShackell5 (1.8k points)

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1 answer 54 views

Determine the oxidation state of the following elements in the compound potassium permanganate (KMnO4): a) Potassium b) Manganese c) Oxygen

asked Feb 4 in ElectroChemistry by Annett65L392 (2.1k points)

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