Recent questions in Chemical thermodynamics

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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 2 days ago in Chemical thermodynamics by BrittneyDivi (570 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 2 days ago in Chemical thermodynamics by LizzieDechai (330 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 2 days ago in Chemical thermodynamics by MinervaElder (610 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 2 days ago in Chemical thermodynamics by Joni19843671 (770 points)

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1 answer 17 views

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 2 days ago in Chemical thermodynamics by SadieTaft39 (610 points)

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1 answer 28 views

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 2 days ago in Chemical thermodynamics by RandalStolle (810 points)

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1 answer 6 views

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 2 days ago in Chemical thermodynamics by RandyMccune2 (580 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 2 days ago in Chemical thermodynamics by RobtLeighton (410 points)

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1 answer 28 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 2 days ago in Chemical thermodynamics by RoxieMatra31 (430 points)

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1 answer 38 views

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 2 days ago in Chemical thermodynamics by CarmenNorthe (550 points)

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1 answer 32 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 2 days ago in Chemical thermodynamics by PUPMora98542 (450 points)

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1 answer 26 views

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 2 days ago in Chemical thermodynamics by MaurineBenes (370 points)

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1 answer 22 views

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 2 days ago in Chemical thermodynamics by Kindra62Z818 (370 points)

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1 answer 27 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 2 days ago in Chemical thermodynamics by KellieBarber (430 points)

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1 answer 31 views

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 2 days ago in Chemical thermodynamics by LillianWirth (290 points)

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1 answer 22 views

Calculate the standard enthalpy change for the neutralization of HCl with NaOH, given that the heat of formation of water is -285.8 kJ/mol, the heat of formation of NaCl is -411.1 kJ/mol, and the initial concentrations of HCl and NaOH are 1.0 M.

asked 2 days ago in Chemical thermodynamics by CatalinaBerg (630 points)

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1 answer 24 views

Calculate the standard enthalpy change for the neutralization of 50.0 mL of 0.100 M hydrochloric acid with 50.0 mL of 0.100 M sodium hydroxide, assuming that the specific heat capacity of the resulting solution is 4.18 J/g °C and the density of the solution is 1.00 g/mL.

asked 2 days ago in Chemical thermodynamics by MurielC91559 (450 points)

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1 answer 24 views

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 temperature of 25°C, given that the specific heat capacity of the resulting solution is 4.18 J/g°C and its density is 1 g/mL.

asked 2 days ago in Chemical thermodynamics by OZGAustin772 (390 points)

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1 answer 30 views

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 2 days ago in Chemical thermodynamics by SanfordRobso (310 points)

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1 answer 24 views

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 2 days ago in Chemical thermodynamics by ElmerAnderse (470 points)

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