Recent questions in ThermoChemistry

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Calculate the standard enthalpy of formation for magnesium oxide (MgO) given the standard enthalpy of formation for magnesium (Mg) is -601.8 kJ/mol and the standard enthalpy of formation for oxygen (O₂) is 0 kJ/mol.

asked 2 days ago in ThermoChemistry by AurelioVos81 (510 points)

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Calculate the standard enthalpy of formation (ΔH°f) of methane (CH4) given the following data: 2H2(g) + O2(g) → 2H2O(l) ΔH°rxn = -572 kJ/mol C(graphite) + O2(g) → CO2(g) ΔH°rxn = -394 kJ/mol Note: The enthalpy of formation of an element in its standard state is zero (0).

asked 2 days ago in ThermoChemistry by TristanMarlo (450 points)

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Calculate the standard enthalpy of formation (ΔH°f) of carbon dioxide (CO2) at 25°C given the following data:CO(g) + 1/2 O2(g) → CO2(g) ΔH° = -283.3 kJ/molC(s) + O2(g) → CO2(g) ΔH° = -393.5 kJ/molΔH°f (C(s)) = 0 kJ/molΔH°f (O2(g)) = 0 kJ/mol

asked 2 days ago in ThermoChemistry by MichaelBolin (370 points)

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Calculate the standard enthalpy of formation (∆Hf) of water (H2O) given the following information: 2H2(g) + O2(g) → 2H2O(l); ∆H = -572 kJ/mol and the standard enthalpy of formation of O2 is 0 kJ/mol.

asked 2 days ago in ThermoChemistry by WendyHenning (490 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 2 days ago in ThermoChemistry by FrancisCropp (430 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 2 days ago in ThermoChemistry by RosalineStar (390 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 2 days ago in ThermoChemistry by QuinnSwank82 (410 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 2 days ago in ThermoChemistry by DeeCarrera9 (430 points)

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Calculate the standard enthalpy change for the reduction of iron(III) oxide to iron using the following balanced chemical equation:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)Given that the standard enthalpy change of formation for Fe2O3(s) is -824.2 kJ/mol, the standard enthalpy change of formation for CO2(g) is -393.5 kJ/mol, and the standard enthalpy change of formation for Fe(s) is 0 kJ/mol. Assume all reactants and products are in their standard states.

asked 2 days ago in ThermoChemistry by KoryLongstaf (330 points)

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Calculate the standard enthalpy change for the reduction of iron (III) oxide using carbon monoxide as the reducing agent, given that the standard enthalpy of formation for iron (III) oxide is -824.2 kJ/mol and the standard enthalpy of formation for carbon monoxide is -110.5 kJ/mol.

asked 2 days ago in ThermoChemistry by PWOMazie102 (650 points)

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Calculate the standard enthalpy change for the formation of ammonia gas from nitrogen gas and hydrogen gas using Hess's Law, given the following equations and their corresponding enthalpy changes:N2(g) + 3H2(g) → 2NH3(g) ∆H = -92.4 kJ/molN2(g) → 2N(g) ∆H = 941 kJ/molH2(g) → 2H(g) ∆H = 436 kJ/mol

asked 2 days ago in ThermoChemistry by IngridMarcha (430 points)

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Calculate the standard enthalpy change (ΔH°) for the reduction of iron(III) oxide (Fe2O3) to iron (Fe) given the following balanced chemical equation:2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g)The enthalpy of formation for Fe2O3(s) is -824.2 kJ/mol and the enthalpy of formation for CO2(g) is -393.5 kJ/mol. All other substances are in their standard state.

asked 2 days ago in ThermoChemistry by BlancheOus03 (650 points)

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1 answer 38 views

Calculate the quantity of heat required to melt 50.0 g of ice at its melting point (0°C). The enthalpy of fusion of water is 6.01 kJ/mol.

asked 2 days ago in ThermoChemistry by JermaineHoag (250 points)

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1 answer 46 views

Calculate the heat required to sublime 34.5 g of dry ice (solid CO2) at a constant temperature and pressure, given that the heat of sublimation of CO2 is 25.2 kJ/mol.

asked Jan 23 in ThermoChemistry by BrooksBaeza (470 points)

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Calculate the heat required to sublime 25 grams of dry ice (CO2) at a temperature of -78.5 °C if the enthalpy of sublimation is 25.2 kJ/mol.

asked Jan 23 in ThermoChemistry by MonicaTweddl (490 points)

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Calculate the heat required to sublime 20.0 grams of dry ice (solid carbon dioxide) at a temperature of -78.5 °C, given the heat of sublimation of CO2 is 25.2 kJ/mol.

asked Jan 23 in ThermoChemistry by FlynnO086966 (350 points)

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1 answer 52 views

Calculate the heat required to sublime 10 grams of dry ice (carbon dioxide) at its melting point (-78.5°C) and convert it to a gas at its boiling point (-57°C). The heat of sublimation of carbon dioxide is 25.2 kJ/mol.

asked Jan 23 in ThermoChemistry by MeriLathrop0 (570 points)

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Calculate the heat required to raise the temperature of a 50 g sample of water from 25°C to 85°C, given that the specific heat capacity of water is 4.184 J/g°C.

asked Jan 23 in ThermoChemistry by HarryPalacio (550 points)

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Calculate the heat required to raise the temperature of 50 grams of water from 20°C to 80°C. The specific heat capacity of water is 4.184 J/g·°C.

asked Jan 23 in ThermoChemistry by TCALora26978 (530 points)

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1 answer 53 views

Calculate the heat required to raise the temperature of 100.0 grams of water from 25°C to 50°C if the specific heat capacity of water is 4.184 J/g°C.

asked Jan 23 in ThermoChemistry by CharoletteTo (550 points)

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