Recent questions in Chemistry

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Calculate the standard enthalpy of formation of water if you know that the standard enthalpy of combustion of hydrogen is -286 kJ/mol and the standard enthalpy of combustion of oxygen is -394 kJ/mol.

asked Feb 3 in Chemical thermodynamics by ZellaSeamon3 (1.6k points)

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1 answer 156 views

Calculate the standard enthalpy of formation of water (H2O) given the following information:- The standard enthalpy of formation of hydrogen gas (H2) is 0 kJ/mol- The standard enthalpy of formation of oxygen gas (O2) is 0 kJ/mol- The standard enthalpy of combustion of hydrogen gas is -286 kJ/mol- The standard enthalpy of combustion of carbon (C) is -394 kJ/mol- The standard enthalpy of combustion of methane gas (CH4) is -890 kJ/mol

asked Feb 3 in ThermoChemistry by ChiKellett4 (1.5k points)

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Calculate the standard enthalpy of formation of water (H2O) given the following information: ΔHf° of H2(g) = 0 kJ/molΔHf° of O2(g) = 0 kJ/molΔHf° of H2O2(l) = -188.2 kJ/mol

asked Feb 3 in ThermoChemistry by Lavonda96B02 (2.3k points)

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1 answer 129 views

Calculate the standard enthalpy of formation of propane (C3H8) given the following data:- Standard enthalpy of formation of CO2(g) = -393.5 kJ/mol- Standard enthalpy of formation of H2O(l) = -285.8 kJ/mol- Standard enthalpy of combustion of propane at constant pressure = -2220.1 kJ/mol

asked Feb 3 in Chemical thermodynamics by NicholasTwm2 (2.0k points)

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1 answer 152 views

Calculate the standard enthalpy of formation of potassium nitrate (KNO3) given the following information:- Heat of combustion of potassium is -468 kJ/mol- Heat of combustion of nitrogen is -940 kJ/mol- Heat of combustion of oxygen is -283.8 kJ/mol- Heat of formation of KNO3 is -383 kJ/mol.

asked Feb 3 in Chemical thermodynamics by MerissaGxv8 (1.7k points)

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1 answer 116 views

Calculate the standard enthalpy of formation of methanol, CH3OH (l), given that the standard enthalpy of combustion of methanol is -726.4 kJ/mol and the standard enthalpy of formation of carbon dioxide and water are -393.5 kJ/mol and -285.8 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by Miguel37A006 (2.3k points)

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1 answer 151 views

Calculate the standard enthalpy of formation of methane gas (CH4) given the standard enthalpies of formation for carbon dioxide (CO2) (-393.5 kJ/mol) and water vapor (H2O) (-241.8 kJ/mol).

asked Feb 3 in ThermoChemistry by LeroyBothwel (1.9k points)

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1 answer 158 views

Calculate the standard enthalpy of formation of methane gas (CH4) given the following data:- ∆H°combustion of methane = -890.36 kJ/mol - ∆H°formation of H2O (l) = -285.8 kJ/mol - ∆H°formation of CO2 (g) = -393.5 kJ/mol

asked Feb 3 in ThermoChemistry by ColumbusU230 (2.4k points)

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1 answer 146 views

Calculate the standard enthalpy of formation of methane (CH4) given the following enthalpy data: C(graphite) + 2H2(g) → CH4(g) ΔH° = -74.8 kJ/mol ΔH°f[C(graphite)] = 0 kJ/molΔH°f[H2(g)] = 0 kJ/mol (Hint: Use Hess's Law and the fact that the standard enthalpy of formation of an element in its most stable state is zero.)

asked Feb 3 in ThermoChemistry by TBHMelaine51 (2.2k points)

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1 answer 114 views

Calculate the standard enthalpy of formation of methane (CH4) given that the standard enthalpies of formation for CO2 and H2O are -393.5 kJ/mol and -285.8 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by CecileHollin (2.3k points)

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1 answer 139 views

Calculate the standard enthalpy of formation of hydrogen fluoride (HF) given the following reactions and enthalpy change values:2H2(g) + O2(g) → 2H2O(g) ΔH° = -484 kJH2(g) + Cl2(g) → 2HCl(g) ΔH° = -184 kJ1/2 F2(g) + H2(g) → HF(g) ΔH° = -273 kJ.

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

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1 answer 143 views

Calculate the standard enthalpy of formation of glucose (C6H12O6) given that the standard enthalpies of combustion for glucose, carbon, and hydrogen are -2803.6 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by MireyaFlaher (1.6k points)

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1 answer 113 views

Calculate the standard enthalpy of formation of ethane (C2H6) given the following bond energies (in kJ/mol):C-C: 347C-H: 413 Note: The equation for the formation of ethane is:C(graphite) + 3H2(g) -> C2H6(g)

asked Feb 3 in ThermoChemistry by MaricelaBevi (1.9k points)

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1 answer 130 views

Calculate the standard enthalpy of formation of carbon dioxide given the following information: - Standard enthalpy of formation of graphite = 0 kJ/mol- Standard enthalpy of formation of oxygen gas = 0 kJ/mol- Enthalpy of combustion of graphite = -393.5 kJ/mol- Enthalpy of combustion of carbon monoxide = -283.0 kJ/mol- Enthalpy of combustion of hydrogen gas = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by AnjaAbt20068 (2.0k points)

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1 answer 120 views

Calculate the standard enthalpy of formation of carbon dioxide gas (CO2) given the following information: C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ/mol H2(g) + 1/2O2(g) → H2O(l) ΔH = -285.8 kJ/mol 2C(s) + 2H2(g) + 5/2O2(g) → 2CO2(g) + 2H2O(l) ΔH = -890.4 kJ/mol

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

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1 answer 87 views

Calculate the standard enthalpy of formation of carbon dioxide from its elements under standard conditions given the following information:- The standard enthalpy of combustion of carbon to CO2 is -393.5 kJ/mol- The standard enthalpy of combustion of hydrogen to H2O is -285.8 kJ/mol- The standard enthalpy of formation of water is -241.8 kJ/mol.Note: The standard enthalpy of formation of an element in its standard state is zero.

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

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1 answer 166 views

Calculate the standard enthalpy of formation of Carbon dioxide (CO2), given the enthalpies of formation of Carbon monoxide (CO) and Oxygen gas (O2) as -110.5 kJ/mol and 0 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by MichelleHall (2.0k points)

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1 answer 126 views

Calculate the standard enthalpy of formation of carbon dioxide (CO2) using the following information:C(graphite) + O2(g) -> CO2(g), ΔH° = -393.5 kJ/molC(graphite) + 2H2(g) -> CH4(g), ΔH° = -74.8 kJ/mol2H2(g) + O2(g) -> 2H2O(l), ΔH° = -572.0 kJ/mol

asked Feb 3 in ThermoChemistry by AleidaSeifer (1.7k points)

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1 answer 112 views

Calculate the standard enthalpy of formation of carbon dioxide (CO2) using the following data:C(graphite) + O2(g) → CO2(g) ΔH° = -393.5 kJ/mol2H2(g) + O2(g) → 2H2O(l) ΔH° = -572.0 kJ/molHint: Use Hess's law to calculate the standard enthalpy of formation of CO2.

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

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1 answer 124 views

Calculate the standard enthalpy of formation of C2H6(g) given the following information: C(s) + O2(g) → CO2(g); ΔH° = -393.5 kJ/mol H2(g) + 1/2 O2(g) → H2O(l); ΔH° = -285.8 kJ/mol 2C(s) + 3H2(g) → C2H6(g); ΔH° = ?

asked Feb 3 in ThermoChemistry by LaunaRxf8120 (1.7k points)

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