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Calculate the entropy change for the reaction of 2 moles of methane gas reacting with 4 moles of oxygen gas to form carbon dioxide gas and water vapor at a constant temperature of 298 K. The reaction is balanced and the standard entropy values for methane, oxygen, carbon dioxide, and water vapor are given as -0.242, 205.16, 213.74, and 188.72 J/K/mol, respectively.

asked Jan 23 in Chemical thermodynamics by JackQ7308746 (2.0k points)

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Calculate the entropy change for the following chemical reaction at 25 °C: 2H2(g) + O2(g) → 2H2O(l) Given that the standard molar entropy of H2(g), O2(g), and H2O(l) are 130.68 J/mol·K, 205.03 J/mol·K and 70.01 J/mol·K respectively.

asked Jan 23 in Chemical thermodynamics by CecileBills (2.2k points)

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Calculate the entropy change for the combustion of methane at a constant temperature and pressure of 298 K and 1 atm, respectively. The balanced equation for the reaction is:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

asked Jan 23 in Chemical thermodynamics by IsraelSeidel (1.3k points)

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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 BelenPickard (2.3k 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 ChasityBelli (2.2k 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 MargueriteWa (1.8k 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 ChloeBodnar (2.0k 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 GlendaNester (1.8k 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 RoderickKyle (2.4k 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 Latonya89F54 (2.2k 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 MoniqueBrins (1.9k 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 SOYRyan09176 (1.6k 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 EvieOconnor (2.3k 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 KathiFatnown (1.6k 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 Murray05Y450 (1.9k 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 PalmaYuille (2.1k 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 BenjaminWenz (2.0k 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 MichelleHall (2.0k 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 JuliannSfd66 (2.0k 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 LeesaJ55672 (1.9k points)

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