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Determine the standard enthalpy of formation of methane (CH4) using Hess's Law, given the following reactions and enthalpy changes: 1. C(graphite) + 2H2(g) -> CH4(g) ΔH1 = -74.6 kJ/mol 2. 2H2(g) + O2(g) -> 2H2O(l) ΔH2 = -571.7 kJ/mol 3. C(graphite) + O2(g) -> CO2(g) ΔH3 = -393.5 kJ/mol.

asked 2 days ago in Chemical thermodynamics by NYBEvonne703 (370 points)

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Determine the standard enthalpy of formation of methane (CH4) given the following information: The standard enthalpy of formation of CO2 and H2O are -393.5 kJ/mol and -285.8 kJ/mol, respectively. The combustion of 0.50 g of methane in a bomb calorimeter resulted in a 1.20°C temperature increase of the surrounding water. The heat capacity of the bomb calorimeter is 5.85 kJ/°C.

asked 2 days ago in Chemical thermodynamics by ShelliDtj184 (510 points)

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Determine the standard enthalpy of formation of ethanol (C2H5OH) given the following information: 1. The combustion of 1 mole of ethanol yields 1367 kJ of heat.2. The standard enthalpy of formation for CO2(g) and H2O(l) are -393.5 kJ/mol and -285.8 kJ/mol, respectively.

asked 2 days ago in Chemical thermodynamics by AlenaHaddon3 (250 points)

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Determine the standard enthalpy of formation for propane (C3H8) using the following values: - C(graphite) + O2(g) → CO2(g) ΔH° = -393.5 kJ/mol- 2H2(g) + O2(g) → 2H2O(l) ΔH° = -572.4 kJ/mol- C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH° = -2220 kJ/mol

asked 2 days ago in Chemical thermodynamics by EffieSneed2 (270 points)

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Determine the standard enthalpy of formation for methane (CH4) using the combustion reactions of methane and hydrogen gas (H2). Given the standard enthalpy of combustion for CH4 is -890.3 kJ/mol and the standard enthalpy of formation for H2O is -285.8 kJ/mol.

asked 2 days ago in Chemical thermodynamics by TheScientist (32.6k points)

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Determine the standard enthalpy of formation for hydrogen chloride gas using the following data:H2(g) + Cl2(g) → 2HCl(g) ΔH = -184.6 kJ/molH2(g) + 1/2O2(g) → H2O(l) ΔH = -285.8 kJ/mol2HCl(g) + O2(g) → 2ClO(g) + H2O(l) ΔH = -518.2 kJ/mol Note: The standard enthalpy of formation for a compound is the change in enthalpy that occurs when one mole of the compound is formed from its constituent elements, with all substances in their standard state at a given temperature (usually 25°C) and pressure (usually 1 atm).

asked 2 days ago in Chemical thermodynamics by LandonZfs700 (510 points)

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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 2 days ago in ThermoChemistry by EddieWhittin (490 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 2 days ago in Chemical thermodynamics by Sharyl671254 (660 points)

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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 2 days ago in Chemical thermodynamics by MaryjoMcReyn (770 points)

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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 2 days ago in Chemical thermodynamics by AjaSchlink05 (510 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 2 days ago in Chemical thermodynamics by ElouiseD7550 (470 points)

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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 2 days ago in Chemical thermodynamics by PhilipMcKeon (290 points)

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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 2 days ago in Chemical thermodynamics by SonjaVanderm (450 points)

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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 2 days ago in Chemical thermodynamics by ElvisHarford (470 points)

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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 2 days ago in Chemical thermodynamics by CharliKeesle (390 points)

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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 2 days ago in Chemical thermodynamics by TrishaPitcai (370 points)

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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 2 days ago in Chemical thermodynamics by InaLewers025 (330 points)

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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 2 days ago in Chemical thermodynamics by Sammy51U3823 (360 points)

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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 2 days ago in Chemical thermodynamics by FaustoRhea01 (410 points)

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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 2 days ago in Chemical thermodynamics by RichSizemore (830 points)

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