Recent questions in Chemistry

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Calculate the Heat of Sublimation of iodine (I2) if 20.0 grams of iodine sublimate at standard temperature and pressure (STP) from a solid to a gas phase absorbing 62.30 kJ of heat energy in the process.

asked Jan 23 in ThermoChemistry by FrederickaCe (350 points)

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1 answer 52 views

Calculate the heat of sublimation for water when 10 g of ice sublimes at standard conditions (1 atm, 25°C)? Given: Heat of fusion of ice is 6.01 kJ/mol; Heat of vaporization of water is 40.67 kJ/mol.

asked Jan 23 in ThermoChemistry by DottyNealy1 (430 points)

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Calculate the heat of sublimation for iodine if 25 g of iodine is heated from its solid form at -110°C to its gaseous form at 184°C. The molar heat capacity of iodine (s) is 54.44 J mol⁻¹ K⁻¹ and the molar heat capacity of iodine (g) is 36.57 J mol⁻¹ K⁻¹. The molar enthalpy of fusion of iodine is 15.52 kJ mol⁻¹.

asked Jan 23 in ThermoChemistry by GroverGreenw (410 points)

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Calculate the heat of neutralization when 50 mL of 1 M HCl(aq) is mixed with 50 mL of 1 M NaOH(aq) at a constant temperature of 25 °C. The specific heat capacity of the solution is 4.18 J/g·°C, and the density of the solution is 1.00 g/mL.

asked Jan 23 in ThermoChemistry by Lorena01B177 (510 points)

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Calculate the heat of neutralization for the reaction of 50 mL of 2.0 M hydrochloric acid and 50 mL of 2.0 M sodium hydroxide. The specific heat capacity of the solution is 4.18 J/g°C and the temperature change is 10°C.

asked Jan 23 in ThermoChemistry by PhilomenaDue (370 points)

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1 answer 56 views

Calculate the heat of mixing when 50g of ethanol (C2H5OH) is added to 200g of water initially at 25°C. Assume the density of water is 1g/mL and the specific heat capacity of water is 4.184J/(g°C). The enthalpy of vaporization of ethanol is 38.56kJ/mol and assume that ethanol-water mixture has a specific heat capacity of 4.2J/(g°C).

asked Jan 23 in ThermoChemistry by MylesLouden (630 points)

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Calculate the heat of mixing when 50.0 mL of 1.00 M HCl is added to 50.0 mL of 1.00 M NaOH at 25°C. The heat capacity of the solution is 4.18 J/(g·°C) and the density of the final solution is 1.00 g/mL. Assume that the heat change is equal to the enthalpy change.

asked Jan 23 in ThermoChemistry by EdmundoFlora (590 points)

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1 answer 49 views

Calculate the heat of mixing when 50 mL of 0.1 M HCl is mixed with 50 mL of 0.1 M NaOH at 25°C. The heat of neutralization for HCl and NaOH is -57.5 kJ/mol.

asked Jan 23 in ThermoChemistry by ReganHannam5 (370 points)

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Calculate the heat of mixing when 25.0 mL of 0.50 M HCl solution is added to 25.0 mL of 0.50 M NaOH solution at 25 °C. The heat capacity of the resulting solution is 4.18 J/g°C and the density is 1.00 g/mL. Assume the heat of reaction is constant at 57.1 kJ/mol.

asked Jan 23 in ThermoChemistry by HubertTritt (530 points)

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Calculate the heat of mixing when 25 grams of ethanol is added to 75 grams of water at 25°C. The heat of mixing of ethanol in water is -4.4 kJ/mol. Assume the densities of ethanol and water to be 0.789 g/mL and 1 g/mL, respectively, and the specific heat of the mixture to be 4.184 J/g°C.

asked Jan 23 in ThermoChemistry by RefugiaGoffa (490 points)

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1 answer 53 views

Calculate the heat of mixing when 100 mL of 1.0 M HCl is mixed with 100 mL of 1.0 M NaOH at 25°C. The specific heat of the resulting solution is 4.18 J/g°C and the final temperature of the solution is 30°C. Assume the heat capacities of HCl, NaOH, and water are negligible.

asked Jan 23 in ThermoChemistry by AlishaCorone (300 points)

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1 answer 10 views

Calculate the heat of mixing when 100 mL of 0.2 M HCl is mixed with 100 mL of 0.1 M NaOH, assuming that the density of the resulting solution is 1 g/mL and the specific heat capacity is 4.18 J/g℃.

asked Jan 23 in ThermoChemistry by KassieNewbig (470 points)

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1 answer 49 views

Calculate the heat of mixing when 100 mL of 0.1 M HCl is mixed with 200 mL of 0.2 M NaOH at 25°C. The specific heat of the solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. Assume that the heat capacity of the solution is equal to that of pure water.

asked Jan 23 in ThermoChemistry by LuciaTapia1 (630 points)

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1 answer 64 views

Calculate the heat of mixing when 100 mL of 0.1 M HCl are added to 100 mL of 0.1 M NaOH at 25°C, given that the specific heat capacity of the resulting solution is 4.18 J g^−1 K^−1 and the density is 1.00 g mL^−1.

asked Jan 23 in ThermoChemistry by ClemmieHeneg (410 points)

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Calculate the heat of mixing (in kJ/mol) when 100 mL of 0.2 M HCl is added to 200 mL of 0.1 M NaOH at 25°C. Assume the density of the resulting solution is 1 g/mL and specific heat capacity is 4.18 J/(g*K). Also, assume the heat capacity of the solution is the same as water.

asked Jan 23 in ThermoChemistry by Francis3099 (410 points)

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1 answer 31 views

Calculate the heat of hydration when 10.0 g of calcium chloride (CaCl2) dissolves in 100 g of water at 25°C. The enthalpy of solution for calcium chloride is -81.5 kJ/mol.

asked Jan 23 in ThermoChemistry by EmmettWester (770 points)

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1 answer 50 views

Calculate the heat of hydration of MgSO4·7H2O if the enthalpy change for dissolving 1 mol of MgSO4 in water is -26.83 kJ/mol, and the enthalpy change for hydrating 1 mol of MgSO4·7H2O with 7 moles of water is -233.80 kJ/mol.

asked Jan 23 in ThermoChemistry by PhilMadigan7 (470 points)

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Calculate the heat of hydration of magnesium sulfate. When 5.00 g of MgSO₄ is mixed with 25.0 mL of water at 25°C, the temperature of the resulting solution rises to 36.5°C. The specific heat of water is 4.18 J/(g•°C), and the density of the resulting solution is 1.03 g/mL.

asked Jan 23 in ThermoChemistry by MadelineColl (770 points)

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1 answer 45 views

Calculate the heat of hydration of magnesium sulfate (MgSO4) given that 4.17 g of MgSO4 is dissolved in 50.0 ml of water at 25°C, and the resulting solution cools from 25°C to 20°C. The specific heat capacity of the solution is 4.18 J/(g·°C), and the density of the solution is 1.00 g/ml. Don't forget to include the units in your final answer.

asked Jan 23 in ThermoChemistry by AbigailValen (370 points)

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Calculate the heat of hydration of CuSO4.5H2O given that the enthalpy change for the reaction CuSO4.5H2O(s) -> CuSO4(s) + 5H2O(l) is -90.6 kJ/mol. Assume that the specific heat of the hydrated salt is 4.2 J/g*K and the density of the solution is 1.05 g/mL.

asked Jan 23 in ThermoChemistry by ThereseWyric (570 points)

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