Recent questions in ThermoChemistry

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Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) if it releases 5184 kJ/mol of energy.

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

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Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) given the standard enthalpies of formation of sucrose, glucose, and fructose are -2220 kJ/mol, -1274 kJ/mol, and -915 kJ/mol respectively.

asked Jan 23 in ThermoChemistry by Sterling80B (2.1k points)

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1 answer 81 views

Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) given that the enthalpy change of hydrolysis for 1 mole of sucrose is -564 kJ/mol.

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

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1 answer 90 views

Calculate the enthalpy change for the hydrolysis of 2 moles of magnesium bromide, MgBr2, in water, given that the standard enthalpy change of formation of magnesium oxide, MgO, is -601.6 kJ/mol and the standard enthalpy change of formation of hydrogen bromide, HBr, is -36.3 kJ/mol.

asked Jan 23 in ThermoChemistry by EmilyUtley95 (1.9k points)

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1 answer 94 views

Calculate the enthalpy change for the hydrolysis of 10 grams of sodium acetate (NaOH) at 25°C, given the following information:- The specific heat capacity of the solution is 4.18 J/(g·°C)- The initial temperature of the solution is 25°C- The final temperature of the solution after hydrolysis is 30°C- The heat evolved by the reaction is 677 J.

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

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1 answer 74 views

Calculate the enthalpy change for the hydrolysis of 0.1 moles of sucrose in water given the following information: - The enthalpy change of the reaction is -564 kJ/mol.- The molar mass of sucrose is 342.3 g/mol.- The reaction is exothermic.

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

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1 answer 87 views

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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1 answer 98 views

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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1 answer 83 views

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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1 answer 79 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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1 answer 99 views

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 109 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 92 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 183 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 101 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 111 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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1 answer 101 views

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 84 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 82 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 88 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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