Recent questions in ThermoChemistry

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Calculate the heat of hydration of copper (II) sulfate pentahydrate given that 5.00 g of the hydrate was dissolved in 100.0 mL of water at 25°C, and the resulting solution temperature increased from 25°C to 30°C. The molar mass of copper (II) sulfate pentahydrate is 249.685 g/mol and the specific heat capacity of water is 4.184 J/g°C.

asked Jan 23 in ThermoChemistry by SylviaPettey (2.4k points)

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Calculate the heat of hydration of 1 mole of anhydrous copper(II) sulfate (CuSO4) when it is dissolved in water to form its hydrated form, CuSO4·5H2O. Given the following information:- Heat of solution of anhydrous CuSO4: -74.9 kJ/mol- Enthalpy change of hydration of CuSO4·5H2O: -245.1 kJ/mol

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

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Calculate the heat of hydration for the reaction where 1 mole of anhydrous copper(II) sulfate reacts with water to form 5 moles of hydrated copper(II) sulfate, given that the enthalpy change for the reaction is -92.2 kJ/mol.

asked Jan 23 in ThermoChemistry by LeifBarrios7 (2.0k points)

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Calculate the heat of hydration for the reaction where 1 mol of anhydrous copper sulfate combines with 5 mol of water to form 1 mol of hydrated copper sulfate given that the enthalpy change of the reaction is -65 kJ/mol.

asked Jan 23 in ThermoChemistry by DannieGuf001 (2.3k points)

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Calculate the heat of hydration for the reaction between anhydrous copper sulfate (CuSO4) and water (H2O), given that the mass of anhydrous copper sulfate used is 10 g and the temperature of the solution increases from 25°C to 35°C. The molar heat of hydration for copper sulfate pentahydrate (CuSO4.5H2O) is -90.1 kJ/mol.

asked Jan 23 in ThermoChemistry by Katja04J6453 (1.8k points)

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Calculate the heat of hydration for the reaction between 1 mol of anhydrous magnesium sulfate and enough water to produce 1 mol of hydrated magnesium sulfate, given that the enthalpy change of the reaction is -108 kJ/mol.

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

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Calculate the heat of hydration for the dissolution of 5.00 grams of magnesium sulfate heptahydrate in 100.0 grams of water, given that the temperature rises from 25.0°C to 30.0°C. The molar mass of magnesium sulfate heptahydrate is 246.48 g/mol and the specific heat capacity of water is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by MOIRoderick9 (1.8k points)

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Calculate the heat of hydration for the compound sodium sulfate (Na2SO4) given that 3 moles of water are released when 1 mole of the compound dissolves in water. The enthalpy of solution for sodium sulfate is -138 kJ/mol, and the enthalpy of hydration for water is -286 kJ/mol.

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

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Calculate the heat of hydration for magnesium ion when 0.5 moles of magnesium chloride is dissolved in 500 ml of water at 25°C. Given that the enthalpy change of solution for magnesium chloride is -641 kJ/mol and the specific heat capacity of water is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by BobBar745884 (1.9k points)

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Calculate the heat of crystallization, in kilojoules per mole, when 50.0 grams of sodium hydroxide (NaOH) is dissolved in 500.0 grams of water at 25⁰C and then cooled to 5⁰C, assuming that all the heat evolved during the process is transferred to the solution. The heat capacity of water is 4.18 J/gK, and the enthalpy of formation of NaOH is -425 kJ/mol.

asked Jan 23 in ThermoChemistry by OliverOtis4 (2.3k points)

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Calculate the heat of crystallization when 10.0 g of sodium acetate trihydrate (NaCH3COO.3H2O) is dissolved in 100.0 mL of water at 25°C and the solution is allowed to cool to 15°C. The specific heat capacity of the solution is 4.18 J/g °C and the density of the solution is 1.0 g/mL. The heat of solution of sodium acetate trihydrate is -7126 J/mol.

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

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Calculate the heat of crystallization of NaOH given that 10 grams of NaOH dissolves in 100 mL of water at 25°C and the resulting solution is cooled to 0°C. The enthalpy of solution of NaOH is -44.5 kJ/mol, and the density of the resulting solution is 1.1 g/mL.

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

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Calculate the heat of crystallization of NaCl if 1786 kJ of heat is released when 5.00 moles of NaCl form from its elements in their standard states.

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

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Calculate the heat of crystallization of 5 moles of calcium chloride, given that the enthalpy change of hydration of calcium ions is –1622 kJ/mol and that of chloride ions is –364 kJ/mol.

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

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Calculate the heat of crystallization of 10 grams of sodium acetate trihydrate (NaC2H3O2•3H2O) when it is cooled from 50°C to 10°C and crystallizes. The specific heat capacity of water is 4.18 J/g°C. The molar mass of sodium acetate is 82.03 g/mol.

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

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Calculate the heat of crystallization in kJ/mol of a substance, given that 100 g of it dissolved in water and cooled from 60°C to 20°C, releasing 5490 J of heat. The molar mass of the substance is 120 g/mol.

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

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Calculate the heat of crystallization for the solidification of 25 grams of a solution containing 10% sucrose (C12H22O11) by mass. The enthalpy of solution for sucrose in water at a given temperature is -5.73 kJ/mol. The molar mass of sucrose is 342.3 g/mol. Assuming that the solution completely solidifies upon cooling, determine the energy released or absorbed in the process.

asked Jan 23 in ThermoChemistry by BrandieB8434 (2.2k points)

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1 answer 82 views

Calculate the heat of crystallization for NaCl from the given data:The enthalpy of fusion of NaCl = 28.3 kJ/mol and the heat capacity of NaCl is approximately constant at 40.0 J/mol.K for temperatures close to room temperature. The melting point of NaCl is 801 °C and the density of the solid NaCl is 2.16 g/cm³.

asked Jan 23 in ThermoChemistry by Samira94683 (2.2k points)

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1 answer 54 views

Calculate the heat of crystallization (in kJ/mol) of NaOH if 25g of NaOH dissolves in 100g of water at 25°C and releases 4.75kJ of heat.

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

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Calculate the heat of combustion for propane gas, C3H8(g), if 12.5 grams of propane are completely burned in excess oxygen gas and the products of reaction are cooled from 700°C to 25°C. The heat capacities of the reactants and products are as follows: C3H8(g): cp = 44.10 J/K O2(g): cp = 29.38 J/K CO2(g): cp = 36.8 J/K H2O(g): cp = 33.6 J/K Assume that the heat capacities of the products and reactants are constant over the temperature range of the reaction and that the heat lost to the surroundings is negligible.

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

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