Recent questions in ThermoChemistry

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Calculate the enthalpy change of isomerization for the reaction of cyclopropane to propene given that the standard enthalpy of formation of cyclopropane is -119.1 kJ/mol and the standard enthalpy of formation of propene is -103.8 kJ/mol. Assume that the enthalpy change of vaporization for both compounds is negligible.

asked Jan 23 in ThermoChemistry by TanyaPridgen (570 points)

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Calculate the enthalpy change of isomerization for the conversion of n-butane to isobutane if the heat of combustion of n-butane is -2657.5 kJ/mol and the heat of combustion of isobutane is -2878.8 kJ/mol.

asked Jan 23 in ThermoChemistry by MarkMyer6121 (290 points)

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Calculate the enthalpy change of isomerization for the conversion of cis-but-2-ene to trans-but-2-ene, given the standard enthalpy of formation for both isomers. Asssume all other conditions remain constant.

asked Jan 23 in ThermoChemistry by LashawnGoose (430 points)

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Calculate the enthalpy change of isomerization for the conversion of cis-but-2-ene to trans-but-2-ene if the enthalpy of formation of cis-but-2-ene is -24.7 kJ/mol and the enthalpy of formation of trans-but-2-ene is -28.6 kJ/mol. The heat of combustion of but-2-ene is -2723 kJ/mol.

asked Jan 23 in ThermoChemistry by EusebiaSweat (670 points)

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Calculate the enthalpy change of isomerization for the conversion of cis-2-butene to trans-2-butene, given that the heat of combustion of cis-2-butene is -3283.1 kJ/mol and the heat of combustion of trans-2-butene is -3336.8 kJ/mol. Assume that the heat of combustion is representative of the enthalpy of formation.

asked Jan 23 in ThermoChemistry by MacFrueh0732 (590 points)

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Calculate the enthalpy change of ionization for magnesium given the following data: Mg(g) → Mg+(g) + e- ΔH1 = +738 kJ/mol Mg+(g) → Mg2+(g) + e- ΔH2 = +1451 kJ/mol

asked Jan 23 in ThermoChemistry by CarltonJjs44 (390 points)

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Calculate the enthalpy change of ionization for hydrogen gas when one mole of H2 gas is ionized to form two moles of H+ ions in the gas phase, given that the enthalpy change of ionization for H(g) is +1312 kJ/mol.

asked Jan 23 in ThermoChemistry by JanaNye81690 (490 points)

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Calculate the enthalpy change of dissolving 5.00 g of NaOH in 100.0 g of water. The temperature of the resulting solution increases from 25.00°C to 31.50°C. The specific heat capacity of the resulting solution is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by JanetHowitt0 (470 points)

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Calculate the enthalpy change of dissolving 10.0 g of sodium hydroxide (NaOH) in 200.0 mL of water at 25°C. Given: the enthalpy of dissolution of NaOH is -44.5 kJ/mol.

asked Jan 23 in ThermoChemistry by KellyeBucher (270 points)

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Calculate the enthalpy change of dissolving 10 grams of NaCl in 100 mL of water, assuming the resultant solution has a density of 1.0 g/mL and assuming that the heat evolved is absorbed by the water. Given: the enthalpy of hydration of NaCl is -787 kJ/mol.

asked Jan 23 in ThermoChemistry by LatiaHipple6 (550 points)

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Calculate the enthalpy change of dissolution when 5 grams of sodium chloride (NaCl) dissolves in 100 mL of water at 25°C. The molar enthalpy of dissolution of sodium chloride is -3.9 kJ/mol.

asked Jan 23 in ThermoChemistry by IsabellaMcNa (520 points)

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Calculate the enthalpy change of dissolution (in kJ/mol) for NaCl in water, given that 1.00 g of NaCl is dissolved in 50.0 mL of water at 25°C. The density of water is 0.997 g/mL and the specific heat capacity of the solution is assumed to be the same as that of water (4.184 J/gK). The molar mass of NaCl is 58.44 g/mol.

asked Jan 23 in ThermoChemistry by PrestonLeddy (390 points)

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Calculate the enthalpy change of desorption of water from a graphite surface if the initial pressure of water is 10 torr and the final pressure is 1 torr at a constant temperature of 300 K. The surface area of the graphite is 50 cm² and the heat of adsorption of water on the surface is -40 kJ/mol.

asked Jan 23 in ThermoChemistry by MathiasHemma (490 points)

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Calculate the enthalpy change of desorption for a solid substance using the given data: The mass of the substance is 2.5 g, and the temperature change during desorption is 25 °C. The heat capacity of the substance is 1.5 J/g·°C. The molar mass of the substance is 150 g/mol. Assume that the desorption process takes place at constant pressure.

asked Jan 23 in ThermoChemistry by LoriMallard3 (590 points)

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Calculate the enthalpy change of combustion for the reaction of methane (CH4) when 1.25 moles of methane is completely burnt in excess oxygen gas at standard conditions, given that the enthalpy change of combustion for methane is -890.3 kJ/mol.

asked Jan 23 in ThermoChemistry by MargueriteBa (620 points)

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1 answer 49 views

Calculate the enthalpy change of combustion for ethane (C2H6) when 5.00 g of ethane is completely burned in excess oxygen gas, given that the standard enthalpy of combustion of ethane is -1560 kJ/mol.

asked Jan 23 in ThermoChemistry by NannetteBene (370 points)

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Calculate the enthalpy change of combustion for ethane (C2H6) given that the standard enthalpy of formation for ethane is -84.68 kJ/mol, the standard enthalpy of formation for CO2 is -393.5 kJ/mol, and the standard enthalpy of formation for H2O is -241.8 kJ/mol.

asked Jan 23 in ThermoChemistry by LouisZ84615 (390 points)

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Calculate the enthalpy change of adsorption when 2.5 moles of nitrogen gas are adsorbed onto 10 g of activated charcoal at 298 K, given that the pressure of nitrogen gas is 1.0 atm. The molar mass of nitrogen is 28 g/mol, and the initial pressure of nitrogen is 0.5 atm.

asked Jan 23 in ThermoChemistry by AlanaEarly83 (490 points)

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Calculate the enthalpy change of adsorption for the adsorption of CO gas on activated carbon at 25°C, given that the equilibrium constant for the reaction is 1.5×10^3 L/mol and the molar density of CO is 1.25 g/L. The surface area of activated carbon used is 50 m^2/g, and the initial pressure of CO is 2.5 atm.

asked Jan 23 in ThermoChemistry by Kerry0848578 (170 points)

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Calculate the enthalpy change involved in the precipitation reaction between 50ml of 0.1 M lead nitrate solution and 50ml of 0.1 M sodium chloride solution at a constant temperature of 25°C. The balanced chemical equation for the reaction is Pb(NO3)2 + 2NaCl → PbCl2 + 2NaNO3. Standard enthalpies of formation for Pb(NO3)2, NaCl, PbCl2, and NaNO3 are -460.56 kJ/mol, -407.33 kJ/mol, -359.57 kJ/mol, and -467.93 kJ/mol respectively.

asked Jan 23 in ThermoChemistry by CalebConti54 (750 points)

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