Recent questions in ThermoChemistry

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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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1 answer 101 views

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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1 answer 133 views

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 Feb 3 in ThermoChemistry by BeatrisSanfo (1.7k points)

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1 answer 163 views

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 Feb 3 in ThermoChemistry by QTHGenevieve (1.7k points)

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1 answer 140 views

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 Feb 3 in ThermoChemistry by CarmellaBibl (2.0k points)

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1 answer 103 views

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 Feb 3 in ThermoChemistry by AlphonsoKirk (2.1k points)

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1 answer 157 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 Feb 3 in ThermoChemistry by MiquelPlx868 (2.3k points)

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1 answer 68 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 Aline0805519 (1.8k points)

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1 answer 73 views

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 HIELucille73 (2.1k points)

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1 answer 79 views

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 LorenaReinha (1.8k points)

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1 answer 73 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 KellieDefazi (1.8k points)

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1 answer 86 views

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 XGJSidney76 (1.4k points)

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1 answer 68 views

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 Sung68J56969 (2.2k points)

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1 answer 79 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 ReinaldoMunz (1.2k points)

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1 answer 73 views

Calculate the heat released when 50 ml of 0.1 M HCl is neutralized with 50 ml of 0.1 M NaOH, assuming that the specific heat capacity of the mixture is 4.18 J/g°C and the density of the final solution is 1.0 g/mL.

asked Jan 23 in ThermoChemistry by Hanna191905 (2.0k points)

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1 answer 86 views

Calculate the heat released when 300 mL of water at 20°C is mixed with 200 mL of ethanol at 25°C. The specific heat capacity of water is 4.18 J/g°C, the specific heat capacity of ethanol is 2.44 J/g°C, and the heat of mixing for water and ethanol is approximately -21 kJ/mol. Assume that both water and ethanol have a density of 1 g/mL and that the final temperature of the mixture is 22°C.

asked Jan 23 in ThermoChemistry by MorrisMcGahe (1.7k points)

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1 answer 90 views

Calculate the heat released when 10.0 g of solid NaOH at 25.0°C is dissolved in 200.0 mL of water also at 25.0°C, given that the heat of crystallization of NaOH is 44.5 kJ/mol and the density of water is 1.00 g/mL.

asked Jan 23 in ThermoChemistry by DanClay0864 (2.1k points)

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1 answer 93 views

Calculate the heat released when 1 mole of ethane (C2H6) is combusted in oxygen gas to form carbon dioxide and water, given the following enthalpy of combustion values: ΔH°comb(C2H6) = -1560 kJ/mol ΔH°comb(O2) = -393.5 kJ/mol ΔH°f(CO2) = -393.5 kJ/mol ΔH°f(H2O) = -285.8 kJ/mol

asked Jan 23 in ThermoChemistry by GingerJ92570 (1.6k points)

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1 answer 93 views

Calculate the heat of sublimation of solid carbon dioxide (dry ice) given that the enthalpy of fusion of solid carbon dioxide is 8.6 kJ/mol and the enthalpy of vaporization of carbon dioxide gas is 22.8 kJ/mol. (Hint: The heat of sublimation of a substance is equal to the sum of its enthalpy of fusion and enthalpy of vaporization.)

asked Jan 23 in ThermoChemistry by Phillipp6306 (2.1k points)

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1 answer 100 views

Calculate the heat of sublimation of solid carbon dioxide (CO2) given that its enthalpy of fusion is 8.44 kJ/mol and its enthalpy of vaporization is 25.2 kJ/mol. The molar mass of CO2 is 44.01 g/mol.

asked Jan 23 in ThermoChemistry by HarryHodgkin (2.2k points)

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