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Calculate the standard enthalpy change of the reaction below at 298K.Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)Given the following standard enthalpies of formation (ΔHf°):ΔHf°[Fe2O3(s)] = -824.2 kJ/molΔHf°[Fe(s)] = 0 kJ/molΔHf°[CO(g)] = -110.5 kJ/molΔHf°[CO2(g)] = -393.5 kJ/mol. Also, calculate the change in standard entropy of the system (ΔS°) and determine whether the reaction is spontaneous or not.

asked Feb 3 in Inorganic Chemistry by SvenJonathan (1.9k points)

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Calculate the standard enthalpy change of the precipitation reaction between 50.0 mL of 0.100 M Pb(NO3)2 and excess 0.100 M NaCl solution at 25°C given that the reaction is Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2(s) + 2NaNO3 (aq) and the enthalpy of formation of NaNO3 (aq) and NaCl (aq) are -467.7 kJ/mol and -411.2 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by SNBBernd7967 (2.3k points)

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Calculate the standard enthalpy change of the oxidation of hydrogen gas (H2) to form water (H2O) at 298 K, given that the standard enthalpy of formation of water is -285.8 kJ/mol and the bond dissociation enthalpy of the H-H bond is 436 kJ/mol.

asked Feb 3 in ThermoChemistry by HenryBorella (2.2k points)

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Calculate the standard enthalpy change of the formation reaction for carbon dioxide (CO2) given the standard enthalpies of formation for carbon monoxide (CO) and oxygen gas (O2) as -110.5 kJ/mol and -249.2 kJ/mol, respectively.

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

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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 following reduction reaction if the standard enthalpy of formation of FeO is -272.0 kJ/mol and that of Fe is 0 kJ/mol.FeO(s) + H2(g) → Fe(s) + H2O(l)

asked Feb 3 in ThermoChemistry by Lourdes26529 (2.1k points)

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Calculate the standard enthalpy change of the following chemical reaction at 298 K given the following bond energies: 2H2(g) + O2(g) --> 2H2O(l) Bond energies: H-H: 432 kJ/mol O=O: 498 kJ/mol O-H: 464 kJ/mol

asked Feb 3 in Physical Chemistry by TawannaHaine (2.3k 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 reduction for the reaction: Fe2O3(s) + 3H2(g) -> 2Fe(s) + 3H2O(l) Given: Standard enthalpy of formation (ΔHf°) of Fe2O3(s) = -822 kJ/mol Standard enthalpy of formation (ΔHf°) of H2O(l) = -286 kJ/mol Standard enthalpy of fusion (ΔHfus) of Fe(s) = 13.81 kJ/mol Standard enthalpy of vaporization (ΔHvap) of H2(g) = 0.449 kJ/mol Standard enthalpy of formation (ΔHf°) of H2(g) = 0 kJ/mol

asked Feb 3 in ThermoChemistry by AdolphI79338 (1.8k points)

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Calculate the standard enthalpy change of reduction for the following reaction: Cu2+(aq) + 2e- -> Cu(s) Given that the standard electrode potential of Cu2+(aq)/Cu(s) is +0.34 V and the standard electrode potential of Ag+(aq)/Ag(s) is +0.80 V.

asked Feb 3 in ThermoChemistry by WandaBalsill (1.3k 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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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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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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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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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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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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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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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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