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Calculate the enthalpy change for the complete combustion of 5 grams of methane gas (CH4) given that the enthalpy of formation for CH4 is -74.8 kJ/mol and the enthalpy of formation for H2O is -285.8 kJ/mol.

asked Jan 23 in ThermoChemistry by JoyGlauert80 (2.0k points)

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Calculate the enthalpy change for the combustion of methane, given the following balanced chemical equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g)The enthalpies of formation for methane, carbon dioxide, and water are -74.8 kJ/mol, -393.5 kJ/mol, and -241.8 kJ/mol respectively.

asked Jan 23 in Chemical thermodynamics by WUWTaylor875 (1.7k points)

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Calculate the enthalpy change for the combustion of methane gas if the standard enthalpies of formation of CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively.

asked Jan 23 in Chemical thermodynamics by TarenSalmond (1.8k points)

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Calculate the enthalpy change for the combustion of methane gas if 10 grams of methane is burned completely in the presence of excess oxygen gas. Given the following balanced chemical equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)The standard enthalpy of formation for methane gas is -74.8 kJ/mol, carbon dioxide gas is -393.5 kJ/mol, and water vapor is -241.8 kJ/mol.

asked Jan 23 in Chemical thermodynamics by Hulda4183859 (2.2k points)

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Calculate the enthalpy change for the combustion of methane gas at standard conditions if 34.0 g of methane is burned completely in oxygen and releases 802 kJ of heat.

asked Jan 23 in ThermoChemistry by Dannie89E20 (2.0k points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) using Hess's Law, given the following equations and enthalpy changes: C(s) + O2(g) → CO2(g), ΔH = -393.5 kJ/mol2H2(g) + O2(g) → 2H2O(l), ΔH = -571.6 kJ/mol CH4(g) + 2O2(g) → CO2(g) + 2H2O(l), ΔH = ?

asked Jan 23 in ThermoChemistry by Alejandra79W (1.9k points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) if 37.0 g of CH4 is completely burned in a bomb calorimeter and the temperature increases by 285.4 K. Assume that the calorimeter has a heat capacity of 4.40 kJ/K and that the combustion reaction is as follows: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l); ΔH=-890.4 kJ/mol. What is the enthalpy change for the combustion of one mole of methane gas?

asked Jan 23 in Chemical reactions by RichieRedric (1.9k points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) at standard conditions using the given relevant thermodynamic data:2H2(g) + O2(g) -> 2H2O(g); ΔH° = -483.7 kJ/molCH4(g) + 2O2(g) -> CO2(g) + 2H2O(g); ΔH° = ?

asked Jan 23 in Chemical thermodynamics by BradyBassett (2.0k points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) at standard conditions given the following information: 4 moles of methane gas is burned in excess oxygen gas (O2) to form carbon dioxide gas (CO2) and liquid water (H2O). The enthalpy change for the combustion of 1 mole of methane gas is -890.4 kJ/mol.

asked Jan 23 in Chemical thermodynamics by ChanteStroh (1.5k points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) at constant pressure, given that the standard enthalpy of formation for CH4 is -74.8 kJ/mol and the balanced chemical equation for the combustion reaction is:CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) The molar enthalpy of formation of CO2 is -393.5 kJ/mol and that of H2O is -285.8 kJ/mol.

asked Jan 23 in Chemical thermodynamics by RobertoMundy (1.7k points)

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Calculate the enthalpy change for the combustion of methane at standard conditions, given the following information:- The enthalpy of formation of CO2(g) is -393.5 kJ/mol.- The enthalpy of formation of H2O(g) is -241.8 kJ/mol.- The enthalpy of formation of CH4(g) is -74.8 kJ/mol.

asked Jan 23 in Chemical reactions by TwylaArledge (1.6k points)

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Calculate the enthalpy change for the combustion of methane (CH4) at constant pressure, given that the heat of formation for methane is -74.9 kJ/mol and the balanced chemical equation is: CH4 (g) + 2O2 (g) -> CO2 (g) + 2H2O (l) The heat of formation for CO2 is -393.5 kJ/mol and the heat of formation for H2O is -285.8 kJ/mol.

asked Jan 23 in Chemical reactions by AdolphI79338 (1.8k points)

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Calculate the enthalpy change for the combustion of 5.67 grams of methane (CH4) if the standard enthalpy of combustion of methane is -890.4 kJ/mol.

asked Jan 23 in Chemical reactions by CorneliusMen (2.2k points)

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Calculate the enthalpy change for the combustion of 2 moles of methane gas (CH4) at constant pressure, given that the standard enthalpy of formation (ΔHf) of methane gas is -74.8 kJ/mol. Express your answer in kilojoules (kJ).

asked Jan 23 in Chemical thermodynamics by NadiaN491716 (2.1k points)

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Calculate the enthalpy change for the combustion of 1 mole of methane gas (CH4) at standard conditions (25°C and 1 atm), given that the standard enthalpy of formation of methane is -74.87 kJ/mol and the standard enthalpy of formation of carbon dioxide (CO2) and water (H2O) are -393.51 kJ/mol and -285.83 kJ/mol, respectively.

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

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Calculate the enthalpy change for the combustion of 1 mole of methane (CH4) gas given that the standard enthalpy of formation of methane is -74.8 kJ/mol, and the standard enthalpies of formation for carbon dioxide (CO2) and water (H2O) are -393.5 kJ/mol and -241.8 kJ/mol respectively. The balanced chemical equation for the reaction is:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)

asked Jan 23 in Chemical thermodynamics by XGJSidney76 (1.4k points)

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Calculate the enthalpy change for the adsorption of nitrogen gas on the surface of activated charcoal, given that the adsorption pressure is 1 atm at a temperature of 298 K. The quantity of nitrogen gas adsorbed is 0.01 moles per gram of charcoal, and the heat of combustion of the same amount of charcoal is -35.4 kJ/mol.

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

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Calculate the enthalpy change for the adsorption of 2.50 moles of methane gas on a zeolite catalyst supported by alumina, given that the temperature of the system decreases from 298 K to 288 K and the pressure is decreased from 100 atm to 75 atm. The initial and final volumes of the gas are 10.0 L and 8.00 L respectively, and the heat capacity of the system is 25 J/K.

asked Jan 23 in ThermoChemistry by ValentinStec (1.9k points)

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1 answer 53 views

Calculate the enthalpy change for dissolving 10 grams of potassium chloride (KCl) in 200 mL of water, assuming the temperature remains constant at 25°C. The molar mass of KCl is 74.5513 g/mol and the specific heat capacity of water is 4.184 J/g·°C.

asked Jan 23 in ThermoChemistry by Precious09K0 (2.0k points)

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Calculate the enthalpy change and the entropy change of the reaction where 2 moles of HCl(g) reacts with 1 mole of CaO(s) to produce 1 mole of CaCl2(s) and 1 mole of H2O(l). Given the bond dissociation enthalpies (in kJ/mol) of H-H is 436, Cl-Cl is 243, H-Cl is 431, and O-H is 463. The standard entropies (in J/mol K) of HCl(g) is 186.9, CaO(s) is 38.2, CaCl2(s) is 223.0, and H2O(l) is 69.9.

asked Jan 23 in Inorganic Chemistry by AmandaRku513 (1.8k points)

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