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Calculate the entropy change for the combustion of methane (CH4) at 298 K and 1 atm pressure, given the standard molar entropies of CH4, H2O (g), and O2 (g) are 186.3 J/K/mol, 188.7 J/K/mol, and 205.0 J/K/mol, respectively. The balanced chemical equation for the reaction is:CH4 (g) + 2 O2 (g) -> CO2 (g) + 2 H2O (g)

asked Jan 23 in Chemical thermodynamics by LinoShearer (530 points)

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Calculate the entropy change (ΔS) for the reaction below at 298 K:2H2(g) + O2(g) → 2H2O(l)Given the standard molar entropy values are:H2(g) = 130.68 J/K molO2(g) = 205.03 J/K molH2O(l) = 69.91 J/K mol

asked Jan 23 in Chemical thermodynamics by AlexandriaCo (570 points)

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Calculate the entropy change (ΔS) for the combustion of methane gas (CH4) at constant pressure and standard conditions, given the following data: C(s) + O2(g) → CO2(g) ΔS° = -394 J/K·mol 2H2(g) + O2(g) → 2H2O(l) ΔS° = -237 J/K·mol CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH° = -802 kJ/mol

asked Jan 23 in Chemical thermodynamics by SpencerRagga (830 points)

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Calculate the entropy change (∆S) when a container of volume 1.0 L is filled with 1.0 mol of ideal gas at a temperature of 300 K and a pressure of 1.0 atm, and then the gas is allowed to expand irreversibly to fill a volume of 2.0 L against a constant external pressure of 0.5 atm at the same temperature.

asked Jan 23 in Physical Chemistry by GDZWillis962 (390 points)

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Calculate the entropy change (∆S) for the reaction of 2 moles of solid NH4Cl with 1 mole of NaOH in a coffee cup calorimeter at a constant temperature of 25°C. The reaction takes place in 100 mL of water and produces 2 moles of NH3 and 1 mole of NaCl in solution. Assume that the specific heat capacity of water is 4.18 J/g·K and that the final solution temperature after the reaction is complete is 25°C.

asked Jan 23 in Chemical thermodynamics by Krystyna23F4 (590 points)

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Calculate the entropy change (∆S) for the reaction between 2.0 moles of hydrogen gas (H2) and 1.0 mole of oxygen gas (O2) at constant pressure and a temperature of 298 K, given the standard molar entropy values for H2 and O2 to be 130.7 J/K•mol and 205.0 J/K•mol, respectively.

asked Jan 23 in ThermoChemistry by Ofelia983738 (270 points)

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Calculate the enthalpy of vaporization of water given the following information: - The boiling point of water is 100°C- The specific heat capacity of liquid water is 4.18 J/g·°C- The specific heat capacity of steam is 1.84 J/g·°C- The heat of fusion of water is 40.7 kJ/mol - The molar mass of water is 18.015 g/mol- The heat capacity of the container is negligible- Assume that the vaporized water behaves ideally and has a constant heat capacity

asked Jan 23 in ThermoChemistry by FranKinchen (690 points)

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Calculate the enthalpy of vaporization of water given that it has a vapor pressure of 1.00 atm at 100°C and its molar enthalpy of vaporization at 373 K is 40.7 kJ/mol.

asked Jan 23 in ThermoChemistry by DessieStopfo (570 points)

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Calculate the enthalpy of vaporization of water at a temperature of 100 degrees Celsius and a pressure of 1 atm, given that the boiling point of water is 100 degrees Celsius and its enthalpy of vaporization at standard conditions (100 degrees Celsius and 1 atm) is 40.7 kJ/mol.

asked Jan 23 in ThermoChemistry by RacheleChewi (570 points)

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Calculate the enthalpy of vaporization for water if 50.0 g of water is completely vaporized at its boiling point (100°C) using 107 kJ/mol as the heat of vaporization of water.

asked Jan 23 in ThermoChemistry by LoriBraund1 (270 points)

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Calculate the enthalpy of vaporization for water given the following information: The boiling point of water is 100°C and its specific heat capacity is 4.18 J/g°C. The density of water at its boiling point is 0.958 g/mL and the heat of fusion for water is 40.7 kJ/mol. The molar mass of water is 18.015 g/mol.

asked Jan 23 in ThermoChemistry by BartTrotter8 (430 points)

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Calculate the enthalpy of vaporization for water at 100 °C, given that the vapor pressure of water is 101.325 kPa and its molar volume is 18.07 L/mol at boiling point.

asked Jan 23 in ThermoChemistry by ThaoCrews506 (210 points)

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Calculate the enthalpy of vaporization for propane given its heat of fusion is 0.513 kJ/mol and heat of vaporization is 15.90 kJ/mol. The molar mass of propane is 44.10 g/mol.

asked Jan 23 in ThermoChemistry by PedroLeitch (230 points)

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Calculate the enthalpy of solution of sodium hydroxide (NaOH) in water, given that the heat absorbed by the solution is 128.0 kJ/mol and the molar concentration of the solution is 0.1 M. Assume that the specific heat capacity of the solution is the same as that of water (4.18 J/g⋅K) and that the density of the solution is 1.00 g/mL.

asked Jan 23 in ThermoChemistry by Sammy51U3823 (360 points)

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Calculate the enthalpy of solution of sodium chloride (NaCl) when 10 grams of NaCl is dissolved in 100 mL of water assuming that the specific heat capacity of the solution is equal to the specific heat capacity of water (4.18 J/g°C) and the temperature change is negligible.

asked Jan 23 in ThermoChemistry by MagnoliaReve (450 points)

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Calculate the enthalpy of solution for the dissolution of 15g of potassium chloride (KCl) in 100g of water (H2O) given that the temperature change was -12.5°C. The enthalpy of fusion for KCl is 17.2 kJ/mol and the specific heat capacity of water is 4.18 J/g•°C.

asked Jan 23 in ThermoChemistry by LacyBastyan (550 points)

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Calculate the enthalpy of solution for dissolving 5 grams of NaCl in 100 mL of water if the final temperature of the solution is 25°C and the initial temperature of the water was 20°C. The enthalpy of fusion of NaCl is -3.0 kJ/mol and the specific heat capacity of the solution is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by MilagroEub10 (590 points)

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Calculate the enthalpy of solution for 10.0 g of potassium chloride (KCl) dissolved in 100 mL of water, given that the temperature of the solution decreases from 25°C to 20°C. Assume the heat capacity of the solution to be 4.184 J/g°C and that there is no heat loss to the surroundings.

asked Jan 23 in ThermoChemistry by UtaReuter96 (510 points)

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Calculate the enthalpy of solution (in kJ/mol) for dissolving 10.0 g of NaOH(s) in 100.0 g of water at 25°C, given that the final temperature of the solution is 28.5°C and the heat capacity of the solution is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by CarrieGabel2 (510 points)

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Calculate the enthalpy of reduction for the reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)given that the standard enthalpy of formation of Fe2O3(s), CO(g), and CO2(g) are -824kJ/mol, -110.5kJ/mol, and -393.5kJ/mol respectively. Assume all reactants and products are in their standard states.

asked Jan 23 in ThermoChemistry by DominickCadw (480 points)

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