Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change (∆H°) of combustion for methane gas (CH4) given that the heat of formation (∆Hf°) for methane is -74.87 kJ/mol and the heat of formation (∆Hf°) for carbon dioxide (CO2) is -393.51 kJ/mol, and the heat of formation (∆Hf°) for water (H2O) is -285.83 kJ/mol.

asked 2 days ago in Chemical thermodynamics by MichellHenni (430 points)

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1 answer 24 views

Calculate the standard enthalpy change (∆H°) for the vaporization of 10 grams of water at 100°C, given that the molar heat of vaporization of water is 40.7 kJ/mol.

asked 2 days ago in Chemical thermodynamics by CarmaHazon9 (730 points)

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1 answer 41 views

Calculate the standard enthalpy change (∆H°) for the reaction: NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l) given the following information: - The enthalpy change of neutralization of HCl(aq) with NaOH(aq) is -55.9 kJ/mol. - The enthalpy of formation of NaCl(s) is -411.2 kJ/mol.- The enthalpy of vaporization of water (H2O) is 40.7 kJ/mol.Assume that the specific heat capacity of the water is 4.18 J/g K and the density of the solution is 1 g/mL.

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

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1 answer 34 views

Calculate the standard enthalpy change (∆H°) for the reaction: 2HCl(aq) + Na2CO3(aq) → CO2(g) + H2O(l) + 2NaCl(aq) given that the standard enthalpy of formation (∆H°f) for NaCl(aq), H2O(l) and CO2(g) are -407.3 kJ/mol, -285.8 kJ/mol and -393.5 kJ/mol respectively.

asked 2 days ago in Chemical thermodynamics by AleishaAltma (550 points)

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1 answer 34 views

Calculate the standard enthalpy change (∆H°) for the reaction that involves the formation of complex [Fe(H2O)6]Cl3 from its constituent ions, given the following information: Fe3+(aq) + 6H2O(l) ⇌ [Fe(H2O)6]3+ ∆Hf° = +123 kJ/mol Cl-(aq) ∆Hf° = -167 kJ/mol

asked 2 days ago in Chemical thermodynamics by TammiW69782 (470 points)

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1 answer 30 views

Calculate the standard enthalpy change (∆H°) for the reaction of the coordination compound [Co(NH3)6]Cl3 (aq) with NaOH (aq) to produce [Co(NH3)6](OH)3 (aq) and NaCl (aq). Given, the standard enthalpy of formation (∆H°f) for [Co(NH3)6]Cl3, [Co(NH3)6](OH)3 and NaCl are -784.8 kJ/mol, -1273.6 kJ/mol and -411.2 kJ/mol, respectively.

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

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1 answer 41 views

Calculate the standard enthalpy change (∆H°) for the reaction between 50.0 mL of 0.100 M hydrochloric acid (HCl) and 50.0 mL of 0.100 M sodium hydroxide (NaOH), given that the temperature change was -5.01°C and the specific heat capacity of the solution is 4.18 J/g°C. The balanced chemical equation for the reaction is:HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)Note: Assume the density of the solutions is 1.00 g/mL and that the specific heat capacity of the solutions is the same as that of water.

asked 2 days ago in Chemical thermodynamics by JereBrock920 (470 points)

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1 answer 37 views

Calculate the standard enthalpy change (∆H°) for the reaction between 25.0 mL of 0.100 M HCl and 25.0 mL of 0.100 M NaOH at 25°C. The density of each solution is 1.00 g/mL and the heat capacity of the solution is 4.18 J/g·°C. The reaction takes place in a calorimeter, and the temperature increase is measured to be 8.47°C.

asked 2 days ago in Chemical thermodynamics by HarlanKittre (270 points)

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1 answer 25 views

Calculate the standard enthalpy change (∆H°) for the precipitation reaction between aqueous solutions of silver nitrate (AgNO3) and sodium chloride (NaCl) to form solid silver chloride (AgCl), given that 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M NaCl were combined in a calorimeter and the temperature change was recorded as -2.5°C.

asked 2 days ago in Chemical thermodynamics by StewartLivin (490 points)

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1 answer 34 views

Calculate the standard enthalpy change (∆H°) for the precipitation reaction between aqueous solutions of lead(II) nitrate [Pb(NO3)2] and potassium iodide (KI) producing solid lead(II) iodide (PbI2) and aqueous potassium nitrate (KNO3) at a temperature of 25°C.

asked 2 days ago in Chemical thermodynamics by MelisaTieman (430 points)

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1 answer 4 views

Calculate the standard enthalpy change (∆H°) for the neutralization reaction of 50.0 mL of 0.100 M HCl with 75.0 mL of 0.0750 M NaOH at a constant pressure of 1 atm and a temperature of 25°C.

asked 2 days ago in Chemical thermodynamics by Erick9612932 (370 points)

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1 answer 36 views

Calculate the standard enthalpy change (∆H°) for the neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) given the following information:- Balanced chemical equation: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)- ∆H°f of NaCl(aq) = -407.3 kJ/mol- ∆H°f of H2O(l) = -285.8 kJ/mol- Heat capacity of the system, Cp = 4.18 J/g.K- Mass of the HCl solution used = 50.0 g- Concentration of HCl solution = 0.100 M- Volume of NaOH solution used = 100.0 mL- Concentration of NaOH solution = 0.200 MAssume that the specific heat of the solution is equal to that of water at 4.18 J/g.K and that the density o

asked 2 days ago in Chemical thermodynamics by Marguerite52 (230 points)

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1 answer 26 views

Calculate the standard enthalpy change (∆H°) for the formation of ammonia (NH3) at 298 K using the following data: N2(g) + 3H2(g) → 2NH3(g) ∆H° = −92.4 kJ/mol Hint: Standard enthalpy change (∆H°) for a reaction is calculated by taking the sum of the standard enthalpies of the products minus the sum of the standard enthalpies of the reactants.

asked 2 days ago in Chemical thermodynamics by IrisHammond9 (470 points)

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1 answer 28 views

Calculate the standard enthalpy change (∆H°) for the following reaction involving liquids:C6H12O6 (s) + 6O2 (g) → 6CO2 (g) + 6H2O (l)

asked 2 days ago in Chemical thermodynamics by Mallory7392 (570 points)

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1 answer 27 views

Calculate the standard enthalpy change (∆H°) for the dissolution reaction of 5.00 grams of sodium chloride (NaCl) in 100.0 mL of water, given that the final temperature of the solution was 25.0°C and the heat capacity of the solution was 4.18 J/g°C. The molar mass of NaCl is 58.44 g/mol and the density of water is 1.00 g/mL.

asked 2 days ago in Chemical thermodynamics by Mckenzie2132 (310 points)

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1 answer 45 views

Calculate the standard enthalpy change (∆H°) for the dissolution of 5.00 g of solid NaOH in 100.0 mL of water, given that the temperature of the solution increased from 25.0°C to 27.5°C. The density of the solution is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/(g°C). The molar mass of NaOH is 40.00 g/mol.

asked 2 days ago in Chemical thermodynamics by MahaliaSchul (570 points)

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1 answer 17 views

Calculate the standard enthalpy change (∆H°) for the dissolution of 5 grams of table salt (NaCl) in water at 298 kelvin. The molar mass of NaCl is 58.44 g/mol and the heat capacity of the solution is 4.18 J/gK.

asked 2 days ago in Chemical thermodynamics by LouieEmmons4 (470 points)

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1 answer 32 views

Calculate the standard enthalpy change (∆H°) for the combustion of methane (CH4(g)) given the balanced equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)(Note: The values of standard enthalpies of formation of CO2(g), H2O(l) and CH4(g) are -393.5 kJ/mol, -285.8 kJ/mol, and -74.8 kJ/mol, respectively)

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

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1 answer 33 views

Calculate the standard enthalpy change (∆H) for the vaporization of 25.0 g of water at its boiling point (100°C) and 1 atm pressure assuming the heat capacity of water to be constant. Given: The heat of vaporization for water is 40.7 kJ/mol and the molar mass of water is 18.015 g/mol.

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

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1 answer 36 views

Calculate the standard enthalpy change ($\Delta H^\circ$) for the dissolution of 10.0 g of sodium hydroxide (NaOH) in 100.0 mL of water assuming that the specific heat capacity of the solution is 4.18 J g$^{-1}$ K$^{-1}$ and that the initial and final temperatures are 25.0$^\circ$C and 35.0$^\circ$C, respectively. The molar mass of NaOH is 40.0 g mol$^{-1}$.

asked 2 days ago in Chemical thermodynamics by WilliamsBorn (230 points)

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