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Calculate the heat of mixing when 100 mL of 0.1 M HCl is mixed with 200 mL of 0.2 M NaOH at 25°C. The specific heat of the solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. Assume that the heat capacity of the solution is equal to that of pure water.

asked Jan 23 in ThermoChemistry by BrittSalas76 (1.8k points)

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Calculate the heat of mixing when 100 mL of 0.1 M HCl are added to 100 mL of 0.1 M NaOH at 25°C, given that the specific heat capacity of the resulting solution is 4.18 J g^−1 K^−1 and the density is 1.00 g mL^−1.

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

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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 CesarSpragg2 (2.1k 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 EloisaLeavit (1.5k 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 FilomenaWago (1.8k 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 SoilaMacviti (1.8k 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 CheryleKirso (2.1k 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 AmelieW70701 (1.7k 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 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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1 answer 65 views

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 formation of water (H2O) given the following bond energies: H-H = 436 kJ/mol, O-H = 463 kJ/mol.

asked Jan 23 in Chemical bonding by CelsaTroiano (1.6k points)

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Calculate the heat of formation of Methane (CH4), given the following enthalpy changes:- Enthalpy change of combustion of methane = -890.4 kJ mol^-1- Enthalpy change of formation of water = -285.8 kJ mol^-1- Enthalpy change of formation of carbon dioxide = -393.5 kJ mol^-1

asked Jan 23 in Chemical bonding by ClydeC545764 (2.2k points)

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Calculate the heat of formation of methane (CH4) given the standard enthalpies of formation of carbon dioxide (CO2), water (H2O), and oxygen gas (O2).

asked Jan 23 in Chemical bonding by FerneSparks (2.3k points)

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