Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change for the neutralization of 50 mL of 0.1 M hydrochloric acid with 50 mL of 0.1 M sodium hydroxide at a constant pressure and a temperature of 25°C. The balanced equation for the reaction is: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

asked Feb 3 in Chemical thermodynamics by AshleighFleg (2.1k points)

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Calculate the standard enthalpy change for the neutralization of 25.0 mL of 1.0 M hydrochloric acid (HCl) with 25.0 mL of 1.0 M sodium hydroxide (NaOH) solution at 25°C, given that the specific heat capacity of the solutions is 4.18 J/g°C, and the density of the solutions is 1.00 g/mL.

asked Feb 3 in Chemical thermodynamics by LannyNewell (1.8k points)

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Calculate the standard enthalpy change for the neutralization of 25 mL of 0.10 M hydrochloric acid with 25 mL of 0.10 M sodium hydroxide. Assume the specific heat capacity of the solution to be 4.18 J/(g*K) and the density of the solution to be 1.00 g/mL. The temperature change observed during the reaction was 4.5°C.

asked Feb 3 in Chemical thermodynamics by GlenCaringto (2.1k points)

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Calculate the standard enthalpy change for the melting of 10 grams of ice at -10°C to liquid water at 20°C, given the specific heat capacity of water is 4.18 J/g°C and the enthalpy of fusion of water is 6.01 kJ/mol.

asked Feb 3 in Chemical thermodynamics by MarielScully (1.4k points)

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Calculate the standard enthalpy change for the liquid-to-gas phase transition of water at 100°C and atmospheric pressure, given that the enthalpy of vaporization of water is 40.7 kJ/mol.

asked Feb 3 in Chemical thermodynamics by JoelPrentice (1.4k points)

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1 answer 88 views

Calculate the standard enthalpy change for the given reaction using the given data:2H2(g) + O2(g) --> 2H2O(l)Given:ΔHf°(H2O(l)) = -285.83 kJ/molΔHf°(O2(g)) = 0 kJ/molΔHf°(H2(g)) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by Denny08T6070 (2.5k points)

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Calculate the standard enthalpy change for the fusion reaction of solid sodium chloride (NaCl) at 25°C, given the following information: ΔHf°[NaCl(s)] = -411 kJ/molΔHf°[Na(s)] = 108 kJ/molΔHf°[Cl2(g)] = 0 kJ/mol The balanced chemical equation for the fusion reaction of NaCl is:NaCl(s) → Na(s) + 1/2Cl2(g)

asked Feb 3 in Chemical thermodynamics by ErnestineScr (1.6k points)

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Calculate the standard enthalpy change for the fusion reaction of solid lithium at its melting point, assuming that the reaction is carried out under standard conditions.

asked Feb 3 in Chemical thermodynamics by UteKqe974841 (1.9k points)

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Calculate the standard enthalpy change for the fusion reaction of a sodium atom. Given the enthalpy of formation of Na(g) is 107.3 kJ/mol and the enthalpy of fusion of Na(s) is 2.6 kJ/mol.

asked Feb 3 in Chemical thermodynamics by Sylvia941924 (1.9k points)

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Calculate the standard enthalpy change for the fusion reaction of 50g of ice at 0°C with 450g of liquid water at 25°C. The molar enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.18 J/g·°C. Assume there are no heat losses to the surroundings.

asked Feb 3 in Chemical thermodynamics by ColinVanderm (2.0k points)

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1 answer 73 views

Calculate the standard enthalpy change for the fusion reaction of 1 mole of ice at 0°C to 1 mole of liquid water at 0°C. Given the standard enthalpy of fusion of water is 6.02 kJ/mol and the specific heat capacity of water is 4.18 J/(g·°C).

asked Feb 3 in Chemical thermodynamics by LewisR691771 (1.8k points)

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Calculate the standard enthalpy change for the fusion of solid silver (Ag) at its melting point (961.78°C) to liquid silver (Ag) at the same temperature. Given the standard enthalpy of fusion of solid silver is 11.3 kJ/mol.

asked Feb 3 in Chemical thermodynamics by NoellaEtx177 (1.7k points)

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Calculate the standard enthalpy change for the fusion of solid hydrogen (H₂) at its melting point of 13.81 K, given that the standard enthalpy of fusion of H₂ is 0.117 kJ/mol.

asked Feb 3 in Chemical thermodynamics by MelbaTulloch (2.2k points)

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Calculate the standard enthalpy change for the fusion of ice at 0°C to liquid water at 0°C, given that the enthalpy of fusion of ice is 6.01 kJ/mol and the molar mass of water is 18.015 g/mol.

asked Feb 3 in Chemical thermodynamics by TawannaPigot (1.5k points)

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Calculate the standard enthalpy change for the fusion of 50 grams of ice at -10°C to liquid water at 10°C. Given the enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.184 J/g°C.

asked Feb 3 in Chemical thermodynamics by SheliaSaucie (2.1k points)

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1 answer 75 views

Calculate the standard enthalpy change for the fusion of 25 grams of ice at -10°C to liquid water at 20°C. The specific heat capacity of ice is 2.09 J/g°C, the specific heat capacity of water is 4.18 J/g°C, and the enthalpy of fusion of water is 6.01 kJ/mol.

asked Feb 3 in Chemical thermodynamics by DoraSturm903 (1.8k points)

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1 answer 62 views

Calculate the standard enthalpy change for the fusion of 2.5 moles of solid sulfur (S8) at its melting point (388 K) using the given information: ΔHfus = 9.73 kJ/mol ΔSfus = 22.8 J/(mol*K) The molar heat capacity of solid sulfur is 22.75 J/(mol*K) and the heat capacity of the liquid sulfur is 37.05 J/(mol*K).

asked Feb 3 in Chemical thermodynamics by MerissaStins (1.8k points)

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Calculate the standard enthalpy change for the fusion of 2.5 moles of ice at 0℃ to form water at 0℃. Given that the molar enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.18 J/g·℃.

asked Feb 3 in Chemical thermodynamics by HowardAlmond (1.8k points)

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Calculate the standard enthalpy change for the fusion of 100 grams of ice at 0°C to liquid water at 0°C. The specific heat capacity of water is 4.184 J/g°C, the standard enthalpy of fusion of water is 6.01 kJ/mol, and the molar mass of water is 18.015 g/mol. Assume all heat absorbed is used to melt the ice and the temperature remains constant.

asked Feb 3 in Chemical thermodynamics by KristiMoore (2.0k points)

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Calculate the standard enthalpy change for the fusion of 1 mole of solid water (ice) at 0°C to liquid water at 0°C. Given the enthalpy of fusion of solid water as 6.01 kJ/mol and the specific heat capacity of water as 4.18 J/g°C.

asked Feb 3 in Chemical thermodynamics by BetteBoniwel (1.6k points)

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