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Calculate the enthalpy of combustion of methane gas (CH4), given that the heat released when 1.0 g of methane completely burns in excess oxygen is -890 kJ.

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

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Calculate the enthalpy of combustion of ethanol (C2H5OH) if 45.1 g of ethanol is burned completely in excess oxygen, producing 145.5 kJ of heat energy.

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

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Calculate the enthalpy of combustion of ethane (C2H6) using the following information: The enthalpy of formation of C2H6 is -84.7 kJ/mol, the enthalpy of formation of CO2 is -393.5 kJ/mol, and the enthalpy of formation of H2O is -241.8 kJ/mol.

asked Jan 23 in ThermoChemistry by Carole803671 (1.8k points)

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Calculate the enthalpy of combustion of butane (C4H10) in kJ/mol given that its heat of formation value is -126.6 kJ/mol and the heat of formation values of CO2 and H2O are -393.5 kJ/mol and -241.8 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry by Karine04K24 (2.0k points)

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1 answer 54 views

Calculate the enthalpy of combustion for sucrose (C₁₂H₂₂O₁₁) given that 5.25 g of sucrose were burned in a bomb calorimeter and the temperature rose by 2.75 °C. The heat capacity of the calorimeter is 20.45 kJ/°C.

asked Jan 23 in ThermoChemistry by IWHJaxon1452 (2.1k points)

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1 answer 64 views

Calculate the enthalpy of adsorption when 2.5 grams of hydrogen gas is adsorbed onto a surface at a temperature of 298 K. The equilibrium pressure of hydrogen gas at this temperature is 1.5 atm and the surface area of the adsorbent is 50 cm². (Assume ideal gas behavior and that the adsorption occurs under standard conditions.)

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

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Calculate the enthalpy of adsorption when 2.0 grams of activated charcoal adsorbs 25 mL of methane gas at a constant temperature of 298 K, given that the pressure is 1 atm. Assume ideal gas behavior for methane.

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

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Calculate the enthalpy of adsorption of nitrogen gas on the surface of activated charcoal at 298 K, given that the equilibrium pressure of nitrogen is 8.5 x 10^-3 atm and the surface area of the charcoal is 1200 m^2/g.

asked Jan 23 in ThermoChemistry by MaynardErb58 (2.0k points)

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1 answer 47 views

Calculate the enthalpy of adsorption of methane gas on activated charcoal at room temperature (25°C) given the following information:- The saturation pressure of methane at 25°C is 3.78 MPa.- The surface area of activated charcoal used is 100 m²/g.- The amount of methane adsorbed on the activated charcoal is 5 mmol/g.

asked Jan 23 in ThermoChemistry by IvyHogan8844 (1.6k points)

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1 answer 60 views

Calculate the enthalpy of adsorption of hydrogen gas on platinum at 298 K, given that the maximum coverage of hydrogen on the platinum surface is 0.5 monolayers and the equilibrium constant for the process at 298 K is 2.5 x 10^3. Assume that the adsorption process is exothermic and that the standard enthalpy of formation of water is -286 kJ/mol.

asked Jan 23 in ThermoChemistry by YOKIva496594 (2.6k points)

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1 answer 51 views

Calculate the enthalpy of adsorption of hydrogen gas on activated carbon if 2 grams of activated carbon absorb 0.025 moles of hydrogen gas at 298 K and the pressure of the system is 1 atm. The molar enthalpy of hydrogen gas is -285.8 kJ/mol at constant pressure.

asked Jan 23 in ThermoChemistry by MaxwellDuff3 (1.9k points)

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1 answer 56 views

Calculate the enthalpy of adsorption of benzene vapor on silica gel at 25°C and a pressure of 2.0 atm, given that the mass of adsorbent used is 0.25 g and the adsorption capacity of silica gel for benzene at this temperature and pressure is 0.75 g/g.

asked Jan 23 in ThermoChemistry by Latonya89F54 (2.2k points)

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Calculate the enthalpy of adsorption of 1 mole of hydrogen gas on the surface of activated charcoal from the given data:- The heat of combustion of hydrogen gas at constant volume is -285.8 kJ/mol- The heat of combustion of hydrogen gas at constant pressure is -241.8 kJ/mol- The heat of vaporization of hydrogen gas at its boiling point (20.3 K) is 0.452 kJ/mol- The surface area of activated charcoal is 500 m²/g- The weight of activated charcoal used is 0.5 g.

asked Jan 23 in ThermoChemistry by BradConger9 (1.8k points)

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1 answer 71 views

Calculate the enthalpy of adsorption for the adsorption of nitrogen gas on activated carbon at 298 K, given that the partial pressure of nitrogen gas is 1.2 atm and the amount of adsorbate adsorbed per gram of adsorbent is 0.45 mol/g. The enthalpy of liquefaction of nitrogen gas at boiling point (-196 °C) is -5.58 kJ/mol.

asked Jan 23 in ThermoChemistry by DanaPittmann (1.5k points)

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Calculate the enthalpy of adsorption for the adsorption of hydrogen gas onto a nickel surface at 25°C, given that the equilibrium pressure of hydrogen gas is 0.5 atm and the surface coverage is 0.2 monolayers. The heat of dissociation of hydrogen gas is 436 kJ/mol.

asked Jan 23 in ThermoChemistry by Melanie86K41 (1.7k points)

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1 answer 69 views

Calculate the enthalpy of adsorption for the adsorption of 5 grams of hydrogen gas on a solid adsorbent at a temperature of 298 K, if the pressure of hydrogen gas is 2.5 atm and the volume of the adsorbent is 100 cm3. Assume ideal gas behavior and use the equation ΔH = -q/n, where ΔH is the enthalpy of adsorption, q is the heat absorbed, and n is the number of moles of gas adsorbed.

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

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1 answer 80 views

Calculate the enthalpy of adsorption for the adsorption of 2.5 moles of nitrogen gas at 298 K on the surface area of 1 gram of activated charcoal, given that the partial pressure of nitrogen gas is 0.1 atm. The heat of vaporization of nitrogen is 5.6 kJ/mol. Express your answer in kJ/mol.

asked Jan 23 in ThermoChemistry by TawannaHaine (2.3k points)

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1 answer 49 views

Calculate the enthalpy of adsorption for a reaction where 2 moles of nitrogen gas (N2) are adsorbed on the surface of a solid at -100°C. Given that the partial pressure of N2 in the gas phase is 0.2 atm and the equilibrium constant for adsorption of N2 at this temperature is 2.5 x 10^3. Assume the adsorption is a reversible process and that the ideal gas law can be used to calculate partial pressures.

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

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1 answer 60 views

Calculate the enthalpy change when solid sodium hydroxide (NaOH) is dissolved into water, given that the desorption enthalpy of NaOH is 44.51 kJ/mol and the molar heat of solution is -44.51 kJ/mol.

asked Jan 23 in ThermoChemistry by LeesaJ55672 (1.9k points)

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1 answer 72 views

Calculate the enthalpy change when 50.0 grams of ammonium nitrate dissolves in 250 mL of water at 25°C. The initial temperature of water was also 25°C and the final temperature after dissolution was 18.5°C. The molar mass of ammonium nitrate is 80.04 g/mol and the specific heat of water is 4.184 J/g°C. Assume that the heat capacity of the solution is the same as that of water.

asked Jan 23 in ThermoChemistry by DominickPlum (2.5k points)

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