Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change of the formation of water (H2O) given the following data:- Standard enthalpy of formation of hydrogen gas (H2) = 0 kJ/mol- Standard enthalpy of formation of oxygen gas (O2) = 0 kJ/mol- Standard enthalpy of formation of water vapor (H2O(g)) = -241.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by Precious09K0 (2.0k points)

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Calculate the standard enthalpy change of the dissolution reaction for 5.00 g of NaOH in 100 mL of water, given the molar heat of solution of NaOH as -44.5 kJ/mol.

asked Feb 3 in Chemical thermodynamics by IeshaC20996 (1.7k points)

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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 Feb 3 in Chemical thermodynamics by AntonioDaven (1.7k points)

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1 answer 48 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 Feb 3 in Chemical thermodynamics by NinaDimattia (1.6k points)

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1 answer 85 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 Feb 3 in Chemical thermodynamics by BrainRubin29 (2.2k points)

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1 answer 70 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 Feb 3 in Chemical thermodynamics by Maura45O7086 (2.5k 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 Feb 3 in Chemical thermodynamics by AdaFennescey (1.8k points)

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1 answer 75 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 Feb 3 in Chemical thermodynamics by 73351052550 (1.9k points)

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1 answer 67 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 Feb 3 in Chemical thermodynamics by BlaineBeasle (2.0k points)

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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 Feb 3 in Chemical thermodynamics by ErnestinaMus (1.9k points)

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1 answer 80 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 Feb 3 in Chemical thermodynamics by SterlingIsr (1.7k points)

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1 answer 49 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 Feb 3 in Chemical thermodynamics by Georgianna69 (2.2k points)

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1 answer 120 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 Feb 3 in Chemical thermodynamics by NorineFelici (1.8k points)

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1 answer 79 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 Feb 3 in Chemical thermodynamics by OnitaLoftus1 (2.3k points)

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1 answer 60 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 Feb 3 in Chemical thermodynamics by LSCJoey08837 (2.2k points)

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1 answer 56 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 Feb 3 in Chemical thermodynamics by AudreaV25265 (2.0k points)

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1 answer 76 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 Feb 3 in Chemical thermodynamics by PDQJenifer7 (2.0k points)

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1 answer 76 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 Feb 3 in Chemical thermodynamics by LeathaOchoa (1.7k points)

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1 answer 52 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 Feb 3 in Chemical thermodynamics by CandraIdk507 (2.4k points)

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1 answer 18 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 Feb 3 in Chemical thermodynamics by DoraSturm903 (1.8k points)

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