Recent questions in ThermoChemistry

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Calculate the enthalpy change for the desorption of water vapor from a silica gel desiccant using the following information:Mass of silica gel desiccant = 5.0 gInitial temperature of silica gel desiccant and water vapor = 25.0 °CFinal temperature after desorption of water vapor = 40.0 °CSpecific heat capacity of silica gel = 1.16 J/g°CHeat absorbed by the calorimeter = -222.4 JAssume all heat absorbed by calorimeter comes solely from the desorption of water vapor.

asked Jan 23 in ThermoChemistry by ClydeC545764 (2.2k points)

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1 answer 54 views

Calculate the enthalpy change for the complete oxidation of 12.5 g of methane gas assuming that all the heat evolved is used to heat up 150 g of water from 25°C to 35°C. The enthalpy of formation of CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry by KennyWenz603 (1.7k points)

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1 answer 56 views

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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1 answer 75 views

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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1 answer 85 views

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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1 answer 54 views

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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1 answer 69 views

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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1 answer 73 views

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 70 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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1 answer 68 views

Calculate the enthalpy change (ΔH) for the isomerization of butene-1 to butene-2, given that the heat of combustion of butene-1 and butene-2 are -2657.7 kJ/mol and -2674.4 kJ/mol, respectively.

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

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1 answer 80 views

Calculate the enthalpy change (ΔH) for the dissolution of 10 grams of NaOH in 100 mL of water, given that the final temperature after mixing is 28°C and the initial temperature of water was 25°C. The specific heat capacity of water is 4.18 J/g°C. The molar mass of NaOH is 40.00 g/mol and the enthalpy of dissolution for NaOH is -44.51 kJ/mol.

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

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1 answer 76 views

Calculate the enthalpy change (in kJ/mol) for the polymerization of ethylene to polyethylene, given that the polymerization of 1 mole of ethylene produces 3 moles of polyethylene and the enthalpy change of the reaction is -32 kJ/mol.

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

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1 answer 66 views

Calculate the enthalpy change (in kJ/mol) for the isomerization reaction of butene-1 to butene-2. Given the standard enthalpy of formation values for butene-1 as -126.3 kJ/mol and butene-2 as -126.0 kJ/mol, and the heat of combustion values for butene-1 as -2670.0 kJ/mol and butene-2 as -2666.0 kJ/mol.

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

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1 answer 86 views

Calculate the enthalpy change (in kJ/mol) for the ionization of sulfuric acid (H2SO4) given the following information: H2SO4 (l) → H+ (aq) + HSO4- (aq)ΔH1 = +1009 kJ/molHSO4- (aq) → H+ (aq) + SO4^2- (aq)ΔH2 = +513 kJ/mol.

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

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1 answer 78 views

Calculate the enthalpy change (in kJ/mol) for the ionization of magnesium, given that the first ionization energy of magnesium is 738 kJ/mol and the second ionization energy is 1450 kJ/mol.

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

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1 answer 51 views

Calculate the enthalpy change (in kJ/mol) for dissolving 10 grams of NaOH in 100 mL of water at 25°C, given that the molar heat of solution for NaOH is -444.6 kJ/mol.

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

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1 answer 80 views

Calculate the enthalpy change (∆H) for the combustion reaction of methane gas (CH4) using Hess’s Law, when the enthalpy changes for the following reactions are given: Reaction 1: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l); ∆H = -891 kJ/mol Reaction 2: C (s) + O2 (g) → CO2 (g); ∆H = -393.5 kJ/mol Reaction 3: 2H2 (g) + O2 (g) → 2H2O (l); ∆H = -484 kJ/mol

asked Jan 23 in ThermoChemistry by SueCasteel38 (1.4k points)

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Calculate the bond dissociation energy required to break a carbon-carbon single bond in methane (CH4).

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

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1 answer 72 views

Calculate the bond dissociation energy of the O-H bond in a water molecule if the enthalpy change for the following reaction is -285.8 kJ/mol:2H2(g) + O2(g) -> 2H2O(l)

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

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1 answer 69 views

Calculate the bond dissociation energy of the O-H bond in a water molecule (H2O) given the enthalpy change for the reaction:H2O (g) → H2 (g) + 1/2 O2 (g)ΔH = +483.6 kJ/mol(Note: the bond dissociation energy represents the energy required to break a bond into its constituent atoms.)

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

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