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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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1 answer 54 views

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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1 answer 50 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 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 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 April242096 (680 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 JudyCottee50 (630 points)

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1 answer 52 views

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 FlorineMmj33 (610 points)

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1 answer 54 views

Calculate the heat of formation of methane (CH4) given the following values: - The standard enthalpy of combustion of methane is -890.3 kJ/mol- The bond energies are as follows: C-H = 413 kJ/mol and C-C = 348 kJ/mol.

asked Jan 23 in Chemical bonding by JamiNovotny2 (590 points)

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1 answer 43 views

Calculate the heat of formation of methane (CH4) given the following thermochemical equations and standard heats of formation:2H2 (g) + O2 (g) → 2H2O (l) ΔH° = -572 kJ/molC (s) + O2 (g) → CO2 (g) ΔH° = -393.5 kJ/molNote: The standard heat of formation of CH4 is -74.8 kJ/mol.

asked Jan 23 in Chemical bonding by Genevieve973 (350 points)

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1 answer 53 views

Calculate the heat of formation of methane (CH4) given the following bond energy values: C-H bond energy = 413 kJ/mol and C-C bond energy = 348 kJ/mol.

asked Jan 23 in Chemical bonding by CrystleHumph (530 points)

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1 answer 61 views

Calculate the heat of formation of methane (CH4) given the enthalpies of formation of H2(g) = 0 kJ/mol and CH3(g) = 120.6 kJ/mol.

asked Jan 23 in Chemical bonding by HassieCooch5 (430 points)

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1 answer 41 views

Calculate the heat of formation of carbon dioxide gas (CO2) given the following bond energies: C=O bond energy is 799 kJ/mol and C-O bond energy is 358 kJ/mol.

asked Jan 23 in Chemical bonding by Margarita30G (490 points)

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1 answer 44 views

Calculate the heat of formation of carbon dioxide (CO2) using the following information: The heat of formation of carbon monoxide (CO) is -110.5 kJ/mol and the heat of formation of water (H2O) is -285.8 kJ/mol.

asked Jan 23 in Chemical bonding by JamesCutler4 (250 points)

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1 answer 55 views

Calculate the heat of formation of carbon dioxide (CO2) given the following information: heat of formation of C(graphite) = 0 kJ/mol, heat of formation of O2(g) = 0 kJ/mol, and heat of combustion of graphite = -393.5 kJ/mol.

asked Jan 23 in Chemical bonding by KarryAutry49 (410 points)

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1 answer 46 views

Calculate the heat of formation of a water molecule from its elements, hydrogen and oxygen gas, given that the standard enthalpy of formation of hydrogen gas is -285.8 kJ/mol and the standard enthalpy of formation of oxygen gas is 0 kJ/mol. Show all your work and explain what the resulting sign of the enthalpy of formation means in terms of the stability of the water molecule.

asked Jan 23 in Chemical bonding by FrancescaShe (530 points)

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