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Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) to gaseous carbon dioxide at 298 K and 1 atm pressure, given that the standard enthalpy of sublimation of solid carbon dioxide is 25.2 kJ/mol.

asked Feb 3 in Chemical thermodynamics by QCMBuford07 (230 points)

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Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) at -78.5°C to gaseous carbon dioxide at 1 atm and 25°C, given the following information: The standard enthalpy of fusion of solid carbon dioxide is 8.4 kJ/mol and the standard enthalpy of vaporization of gaseous carbon dioxide is 22.1 kJ/mol.

asked Feb 3 in Chemical thermodynamics by HildredCampo (250 points)

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Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) at -78.5°C to gaseous carbon dioxide at 1 atm and 25°C given that the enthalpy of formation of solid carbon dioxide and gaseous carbon dioxide are -393.5 kJ/mol and -393.5 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by FloridaM0355 (510 points)

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Calculate the standard enthalpy change for the phase transition reaction of solid calcium carbonate (CaCO3) to gaseous carbon dioxide (CO2) at 298 K, given the following formation enthalpies: ΔHf°(CaCO3) = -1206.9 kJ/mol ΔHf°(CO2) = -393.5 kJ/mol Also, assume that the specific heat capacity of CaCO3 is 0.82 J/g·K and that of CO2 is 0.85 J/g·K.

asked Feb 3 in Chemical thermodynamics by BradfordKins (430 points)

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Calculate the standard enthalpy change for the phase transition reaction of solid ammonium nitrate (NH4NO3) to gaseous NH3 and NO2, given that the standard enthalpy of formation for solid NH4NO3 is -365.5 kJ/mol, the standard enthalpy of formation for NH3(g) is -46.1 kJ/mol, and the standard enthalpy of formation for NO2(g) is 33.2 kJ/mol.

asked Feb 3 in Chemical thermodynamics by HarryWcc2527 (490 points)

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Calculate the standard enthalpy change for the phase transition reaction of ice to water at a constant pressure of 1 atm, given the following information:- The standard enthalpy of fusion for ice is 6.01 kJ/mol.- The molar heat capacity of ice is 36.8 J/(mol K).- The molar heat capacity of liquid water is 75.3 J/(mol K).- The melting point of ice is 0°C.- The boiling point of water is 100°C.

asked Feb 3 in Chemical thermodynamics by SanfordRobso (710 points)

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Calculate the standard enthalpy change for the phase transition reaction from solid to liquid for a sample of substance X, given that the mass of the sample is 10 grams and the melting point of substance X is 50°C. The specific heat capacity of substance X is 2 J/g°C and the enthalpy of fusion for substance X is 50 J/g.

asked Feb 3 in Chemical thermodynamics by NiklasRay943 (170 points)

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Calculate the standard enthalpy change for the phase transition of water from liquid to ice at 0°C, given the following information: The molar heat capacity of liquid water, Cp = 75.3 J/mol K The molar heat capacity of ice, Cp = 36.6 J/mol K The enthalpy of fusion, ΔHfus = 6.01 kJ/mol

asked Feb 3 in Chemical thermodynamics by CorneliusSpe (470 points)

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Calculate the standard enthalpy change for the phase transition of solid ice to liquid water, given the heat of fusion of ice is 6.01 kJ/mol and the molar heat capacity of water is 75.3 J/mol·K.

asked Feb 3 in Chemical thermodynamics by Willis55N919 (430 points)

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Calculate the standard enthalpy change for the phase transition of solid copper to liquid copper given the following data: - the melting point of copper is 1,085°C - the molar heat of fusion of copper is 13.1 kJ/mol.

asked Feb 3 in Chemical thermodynamics by AletheaFiori (490 points)

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Calculate the standard enthalpy change for the phase transition of ice to water at 298 K, given that the heat of fusion of ice is 6.01 kJ/mol and the molar heat capacity of ice and water are 37.0 J/(mol*K) and 75.3 J/(mol*K), respectively.

asked Feb 3 in Chemical thermodynamics by MarjorieChad (410 points)

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Calculate the standard enthalpy change for the neutralization reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH) when 50.0 mL of 1.0 M HCl reacts with 50.0 mL of 1.0 M NaOH in a constant pressure calorimeter. Assume the density of the final solution is the same as that of pure water (1 g/mL) and that the specific heat capacity of the final solution is 4.18 J/g K.

asked Feb 3 in Chemical thermodynamics by CoraBaehr282 (230 points)

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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid and sodium hydroxide, given the balanced chemical equation: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) and the enthalpy change of formation values: ∆Hf°(NaCl(aq)) = -407.3 kJ/mol ∆Hf°(H2O(l)) = -285.83 kJ/mol ∆Hf°(HCl(aq)) = -167.2 kJ/mol ∆Hf°(NaOH(aq)) = -469.11 kJ/mol

asked Feb 3 in Chemical thermodynamics by ClariceOrozc (330 points)

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1 answer 31 views

Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given the balanced chemical equation: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l). The enthalpies of formation for NaCl(aq) and H2O(l) are -407.3 kJ/mol and -285.8 kJ/mol, respectively. The specific heat capacity of the solution is 4.18 J/(g*K), and the mass of the resulting solution is 100 g.

asked Feb 3 in Chemical thermodynamics by MattieMabry8 (470 points)

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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given the appropriate thermochemical equations and the following information:- Heat evolved during the reaction, Q = -58.35 kJ/mol- Moles of HCl used, n(HCl) = 0.05 mol- Concentration of NaOH solution, c(NaOH) = 2 M- Volume of NaOH solution used, V(NaOH) = 25.0 mL (assuming density of 1.00 g/mL)Show your calculations and include units in your final answer.

asked Feb 3 in Chemical thermodynamics by Tiffany67L85 (490 points)

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1 answer 34 views

Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), given that the reaction produces water and sodium chloride as products. The molar enthalpy of formation for water is -285.8 kJ/mol and for NaCl is -411.2 kJ/mol. The balanced chemical equation for the reaction is: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

asked Feb 3 in Chemical thermodynamics by LaurenMacon (550 points)

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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) using the following information:- The standard enthalpy of formation for HCl is -92.31 kJ/mol - The standard enthalpy of formation for NaOH is -469.11 kJ/mol The balanced equation for the reaction is:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)

asked Feb 3 in Chemical thermodynamics by BlancaTowns9 (470 points)

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Calculate the standard enthalpy change for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) in aqueous solutions. The balanced chemical equation for the reaction is as follows:HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) Given the enthalpy of formation for HCl(aq) is -167.2 kJ/mol, NaOH(aq) is -469.14 kJ/mol, NaCl(aq) is -407.3 kJ/mol, and H2O(l) is -285.83 kJ/mol. The reaction is carried out at standard temperature and pressure.

asked Feb 3 in Chemical thermodynamics by ThereseWyric (370 points)

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1 answer 28 views

Calculate the standard enthalpy change for the neutralization reaction between 50.0 mL of 0.100 M hydrochloric acid and 75.0 mL of 0.080 M sodium hydroxide. Given: the specific heat capacity of the solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. The balanced chemical equation for the reaction is HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l).

asked Feb 3 in Chemical thermodynamics by ClaritaCress (670 points)

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Calculate the standard enthalpy change for the neutralization of hydrochloric acid (HCl) with sodium hydroxide (NaOH) in aqueous solution when 50.0 mL of 0.100 M HCl was used and 75.0 mL of 0.075 M NaOH was added. Assume that the specific heat capacity of the solution is 4.18 J/g·K and the density of the solution is 1.00 g/mL.

asked Feb 3 in Chemical thermodynamics by MarilouTafoy (630 points)

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