Recent questions in ThermoChemistry

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Calculate the heat of mixing (in kJ/mol) when 100 mL of 0.2 M HCl is added to 200 mL of 0.1 M NaOH at 25°C. Assume the density of the resulting solution is 1 g/mL and specific heat capacity is 4.18 J/(g*K). Also, assume the heat capacity of the solution is the same as water.

asked Jan 23 in ThermoChemistry by Francis3099 (410 points)

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Calculate the heat of hydration when 10.0 g of calcium chloride (CaCl2) dissolves in 100 g of water at 25°C. The enthalpy of solution for calcium chloride is -81.5 kJ/mol.

asked Jan 23 in ThermoChemistry by EmmettWester (770 points)

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Calculate the heat of hydration of MgSO4·7H2O if the enthalpy change for dissolving 1 mol of MgSO4 in water is -26.83 kJ/mol, and the enthalpy change for hydrating 1 mol of MgSO4·7H2O with 7 moles of water is -233.80 kJ/mol.

asked Jan 23 in ThermoChemistry by PhilMadigan7 (470 points)

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Calculate the heat of hydration of magnesium sulfate. When 5.00 g of MgSO₄ is mixed with 25.0 mL of water at 25°C, the temperature of the resulting solution rises to 36.5°C. The specific heat of water is 4.18 J/(g•°C), and the density of the resulting solution is 1.03 g/mL.

asked Jan 23 in ThermoChemistry by MadelineColl (770 points)

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Calculate the heat of hydration of magnesium sulfate (MgSO4) given that 4.17 g of MgSO4 is dissolved in 50.0 ml of water at 25°C, and the resulting solution cools from 25°C to 20°C. The specific heat capacity of the solution is 4.18 J/(g·°C), and the density of the solution is 1.00 g/ml. Don't forget to include the units in your final answer.

asked Jan 23 in ThermoChemistry by AbigailValen (370 points)

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Calculate the heat of hydration of CuSO4.5H2O given that the enthalpy change for the reaction CuSO4.5H2O(s) -> CuSO4(s) + 5H2O(l) is -90.6 kJ/mol. Assume that the specific heat of the hydrated salt is 4.2 J/g*K and the density of the solution is 1.05 g/mL.

asked Jan 23 in ThermoChemistry by ThereseWyric (570 points)

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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 Breanna4436 (550 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 AnnettSheppa (510 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 Beulah10W886 (610 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 PWOMazie102 (650 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 Nydia78K370 (530 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 DerekMcQuay (550 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 AlbertinaSpe (410 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 Dell11H9211 (470 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 MargheritaMa (530 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 XavierLeeper (370 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 Raphael64O24 (690 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 KristinaBeam (590 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 ClarissaBeac (370 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 FloreneTebbu (430 points)

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