Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change of formation of magnesium oxide (MgO) using the following data: ΔH°f for Mg (s) = 0 kJ/molΔH°f for O₂ (g) = 0 kJ/mol ΔH°c for MgO (s) = -601.8 kJ/mol

asked 2 days ago in Chemical thermodynamics by Bradley53M38 (490 points)

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1 answer 16 views

Calculate the standard enthalpy change of formation for the compound methane (CH4) given the following information:- The standard enthalpy change of formation for carbon dioxide (CO2) is -393.5 kJ/mol.- The standard enthalpy change of formation for water (H2O) is -285.8 kJ/mol.- The enthalpy of combustion for methane is -890.4 kJ/mol.

asked 2 days ago in Chemical thermodynamics by FredricPalum (550 points)

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1 answer 35 views

Calculate the standard enthalpy change of formation for ethanoic acid, given the following standard enthalpy of combustion data:- Ethanol: -1367 kJ/mol- Carbon dioxide: -393.5 kJ/mol- Water: -285.8 kJ/molThe chemical equation for the formation of ethanoic acid is:2C2H5OH + 2O2 → 2CH3COOH + 2H2O

asked 2 days ago in Chemical thermodynamics by DuaneLogue13 (290 points)

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1 answer 23 views

Calculate the standard enthalpy change for the vaporization reaction of 25.0 g of water at its boiling point of 100°C using the following information: the molar heat of vaporization of water is 40.7 kJ/mol and the molar mass of water is 18.015 g/mol.

asked 2 days ago in Chemical thermodynamics by FerdinandSid (330 points)

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Calculate the standard enthalpy change for the vaporization reaction of 25.0 g of water at 100°C and atmospheric pressure (1 atm).

asked 2 days ago in Chemical thermodynamics by SheliaGerste (450 points)

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1 answer 31 views

Calculate the standard enthalpy change for the vaporization reaction of 2.00 moles of water at 100°C and 1 atm pressure, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by LottieWolken (550 points)

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1 answer 24 views

Calculate the standard enthalpy change for the vaporization of water at its normal boiling point of 100 degrees Celsius and a pressure of 1 atm. The molar enthalpy of vaporization for water is 40.7 kJ/mol. What is the amount of heat required to vaporize 100 g of water?

asked 2 days ago in Chemical thermodynamics by ChassidyMcCo (490 points)

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1 answer 19 views

Calculate the standard enthalpy change for the vaporization of 25.0 grams of water at 100°C, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by AlbertoLarna (550 points)

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1 answer 17 views

Calculate the standard enthalpy change for the vaporization of 25.0 g of water at 100°C, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol. (The molar mass of water is 18.015 g/mol.)

asked 2 days ago in Chemical thermodynamics by ENCIsabel625 (630 points)

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1 answer 18 views

Calculate the standard enthalpy change for the vaporization of 25.0 g of water at 100°C, given that the molar enthalpy of vaporization is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by LillieIst935 (310 points)

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1 answer 35 views

Calculate the standard enthalpy change for the vaporization of 25 grams of water at 100 degrees Celsius and 1 atmosphere of pressure, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by JewelMoncrie (350 points)

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1 answer 36 views

Calculate the standard enthalpy change for the vaporization of 25 g of liquid nitrogen at its boiling point assuming constant pressure is 1 atm. Given the molar heat of vaporization of nitrogen is 5.56 kJ/mol.

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

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1 answer 22 views

Calculate the standard enthalpy change for the vaporization of 15 grams of water given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by AllieNoyes3 (410 points)

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1 answer 29 views

Calculate the standard enthalpy change for the vaporization of 15 grams of water at its boiling point, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by AstridCrooke (410 points)

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1 answer 26 views

Calculate the standard enthalpy change for the vaporization of 100 g of water at 100°C given that the enthalpy of vaporization of water is 40.7 kJ/mol.

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

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1 answer 25 views

Calculate the standard enthalpy change for the vaporization of 10 grams of water at 100°C, given that the enthalpy of vaporization for water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by IngridMarcha (430 points)

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1 answer 22 views

Calculate the standard enthalpy change for the vaporization of 1 mole of water at 100°C, given that the enthalpy of fusion of water is 6.01 kJ/mol and the enthalpy of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by ValeriaMetca (450 points)

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1 answer 3 views

Calculate the standard enthalpy change for the vaporization of 1 mole of water at 100°C and 1 atm pressure. The enthalpy of formation of liquid water is -285.8 kJ/mol and the enthalpy of formation of water vapor is -241.8 kJ/mol.

asked 2 days ago in Chemical thermodynamics by SheriFkw4940 (630 points)

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1 answer 32 views

Calculate the standard enthalpy change for the transition of liquid water at 100°C to steam at the same temperature, given that the enthalpy of vaporization of water is 40.7 kJ mol-1.

asked 2 days ago in Chemical thermodynamics by AurelioMetts (450 points)

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1 answer 20 views

Calculate the standard enthalpy change for the sublimation of iodine, given that the sublimation of 1 mole of iodine requires 62.44 kJ of energy and the standard enthalpy of formation of iodine (s) is 0 kJ/mol.

asked 2 days ago in Chemical thermodynamics by Kristian7404 (470 points)

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