Recent questions in Chemistry

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Calculate the enthalpy change for the hydrolysis of 0.025 moles of ethyl acetate (C4H8O2) in the presence of excess water, given that the enthalpy of reaction is -56.0 kJ/mol.

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

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Calculate the enthalpy change for the hydration of MgSO4 using the following data:MgSO4(s) → MgSO4(aq) ΔH1 = 44.5 kJ/molMgSO4(aq) + 7H2O(l) → MgSO4 • 7H2O(s) ΔH2 = -63.2 kJ/mol.

asked Jan 23 in ThermoChemistry by MistyReagan2 (1.4k points)

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Calculate the enthalpy change for the fusion of 50.0 g of ice at its melting point (0 °C). The molar enthalpy of fusion of water is 6.01 kJ/mol.

asked Jan 23 in ThermoChemistry by EttaRide758 (1.3k points)

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Calculate the enthalpy change for the following reaction:2H2O2(aq) → 2H2O(l) + O2(g)Using the following information:2H2O(l) + 105.2 kJ → 2H2(g) + O2(g)2H2(g) + O2(g) → 2H2O2(aq) + 484.4 kJ

asked Jan 23 in Chemical reactions by LuzMccrary7 (2.5k points)

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Calculate the enthalpy change for the following reaction, using Hess's Law:2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)Given the following enthalpy changes: 2H2(g) + O2(g) → 2H2O(l) ΔH1 = -484 kJ2SO2(g) + O2(g) → 2SO3(g) ΔH2 = -198 kJ2H2(g) + S(s) → H2S(g) ΔH3 = +25kJ

asked Jan 23 in Chemical reactions by BelenPickard (2.3k points)

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1 answer 61 views

Calculate the enthalpy change for the following reaction using Hess's Law: 2SO3(g) → 2SO2(g) + O2(g)Given the following enthalpy changes:2SO3(g) + ΔH1 → 2SO2(g) + O2(g); ΔH1 = 198.2 kJ/molSO2(g) + 1/2O2(g) + ΔH2 → SO3(g); ΔH2 = -98.9 kJ/mol

asked Jan 23 in Chemical reactions by CarmaC633252 (1.7k points)

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1 answer 43 views

Calculate the enthalpy change for the following reaction using Hess's Law calculations:2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)Given the following information:2H2(g) + O2(g) → 2H2O(l) ΔH1 = -484 kJ/mol2S(s) + 3O2(g) → 2SO3(g) ΔH2 = -791 kJ/mol2H2(g) + S(s) → 2H2S(g) ΔH3 = -36 kJ/mol

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

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Calculate the enthalpy change for the following polymerization reaction: 2 C2H4 (g) → C4H8 (g) Given the following bond enthalpies: C-H = 413 kJ/mol, C-C = 348 kJ/mol, C=C = 611 kJ/mol Assume all reactants and products are gases at 298 K and 1 atm.

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

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1 answer 13 views

Calculate the enthalpy change for the following combustion reaction:C2H6(g) + 7/2 O2(g) --> 2CO2(g) + 3H2O(l)Using the following reactions and their corresponding enthalpies of formation:C2H6(g) + 3 1/2 O2(g) --> 2CO2(g) + 3H2O(l) ΔH°f = -1560 kJ/mol2H2(g) + O2(g) --> 2H2O(l) ΔH°f = -484 kJ/mol.

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

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1 answer 76 views

Calculate the enthalpy change for the following chemical reaction:2H2(g) + O2(g) -> 2H2O(l) given the following bond enthalpy values:H-H bond energy = 436 kJ/mol O=O bond energy = 498 kJ/mol H-O bond energy = 464 kJ/mol

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

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Calculate the enthalpy change for the following chemical reaction: 2NH3(g) + 3O2(g) → 2NO(g) + 3H2O(l) Given the following enthalpy values: ΔH°f (NH3) = −46.11 kJ/molΔH°f (O2) = 0 kJ/molΔH°f (NO) = 90.3 kJ/molΔH°f (H2O) = −285.8 kJ/mol

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

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1 answer 64 views

Calculate the enthalpy change for the dissolution of 5.00 g of sodium hydroxide (NaOH) in 100.0 g of water (H2O). The temperature change was measured to be -3.45°C. Given that the specific heat of water is 4.18 J/g°C and the density of water is 1.00 g/mL. (Assume that the heat evolved from NaOH is absorbed by the water.)

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

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1 answer 101 views

Calculate the enthalpy change for the dissolution of 5.00 g of potassium chloride (KCl) in 100 mL of water. Given that the specific heat capacity of the resulting solution is 4.18 J/g°C, and its temperature increases from 25.0°C to 30.0°C. The molar mass of KCl is 74.55 g/mol, and the enthalpy of hydration of K+ and Cl- ions is -716 and -364 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry by WandaBalsill (1.3k points)

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1 answer 78 views

Calculate the enthalpy change for the dissolution of 5 grams of sodium chloride in 50 mL of water if the temperature of the solution decreases from 25 °C to 21 °C. The density of the solution is 1.0 g/mL and the specific heat capacity of the solution is 4.18 J/g°C. (Assume the heat exchange between the solution and the surroundings is negligible)

asked Jan 23 in ThermoChemistry by CarmaC633252 (1.7k points)

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1 answer 54 views

Calculate the enthalpy change for the dissolution of 10g of NaCl in 100g of water, given that the initial and final temperatures are 25°C and 20°C respectively. The molar mass of NaCl is 58.44 g/mol and the specific heat capacity of water is 4.18 J/(g°C).

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

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Calculate the enthalpy change for the dissolution of 10.0 grams of sodium chloride (NaCl) in 100 mL of water at 25°C. The density of water is 1.00 g/mL and the heat capacity of the solution is 4.18 J/g°C. The molar mass of NaCl is 58.44 g/mol and its enthalpy of dissolution is -3.9 kJ/mol.

asked Jan 23 in ThermoChemistry by AlmedaGooch6 (1.7k points)

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1 answer 64 views

Calculate the enthalpy change for the dissolution of 10 grams of sodium hydroxide in excess water, given that the solution formed has a final temperature of 25°C, and the specific heat capacity of the solution is 4.184 J/(g°C). The molar enthalpy of dissolution of NaOH is -44 kJ/mol. Assume that the density of the solution is equal to that of water.

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

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1 answer 54 views

Calculate the enthalpy change for the dissolution of 10 g of sodium hydroxide in 100 g of water at a temperature of 25°C, given that the final temperature of the solution is 26.5°C and the specific heat capacity of the solution is 4.18 J g⁻¹ K⁻¹. (Assume that the heat released is absorbed by the solution and there is no heat lost to the surroundings.)

asked Jan 23 in ThermoChemistry by Beatris09Q13 (1.9k points)

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1 answer 59 views

Calculate the enthalpy change for the dissolution of 10 g of NaOH in 100 mL of water at 25°C. The molar heat of dissolution of NaOH is -44.51 kJ/mol.

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

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1 answer 60 views

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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