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The salt magnesium chloride is soluble in water. When 0.530 g of MgCl, is dissolved in 106.00 g of water, the temperature of the solution increases from 25.00 to 26.94 °C. Based on this observation, calculate the enthalpy of dissolution of MgCl, (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. AH dissolution kJ/mol

The salt magnesium chloride is soluble in water. When 0.530 g of MgCl, is dissolved in 106.00 g of water, the temperature of the solution increases from 25.00 to 26.94 °C. Based on this observation, calculate the enthalpy of dissolution of MgCl, (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. AH dissolution kJ/mol

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 24E: A 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the...
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The salt magnesium chloride is soluble in water. When 0.530 g of MgCl, is dissolved in 106.00 g of water, the temperature of the solution increases from 25.00 to 26.94 °C. Based on this observation, calculate the enthalpy of dissolution of MgCl, (in kJ/mol). 6. Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. AH dissolution kJ/mol
Transcribed Image Text:The salt magnesium chloride is soluble in water. When 0.530 g of MgCl, is dissolved in 106.00 g of water, the temperature of the solution increases from 25.00 to 26.94 °C. Based on this observation, calculate the enthalpy of dissolution of MgCl, (in kJ/mol). 6. Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. AH dissolution kJ/mol
A 0.485-g sample of 1,8-0ctanediol (C3H1802) is burned in a bomb calorimeter and the temperature increases from 24.10 °C to 27.20 °C. The calorimeter contains 1.06×10³ g of water and the bomb has a heat capacity of 873 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 1,8-octanediol burned (kJ/mol). C3H1802(s) + 23/2 O2(g) –→8 CO2(g) + 9 H20(1) ΔΕ- kJ/mol
Transcribed Image Text:A 0.485-g sample of 1,8-0ctanediol (C3H1802) is burned in a bomb calorimeter and the temperature increases from 24.10 °C to 27.20 °C. The calorimeter contains 1.06×10³ g of water and the bomb has a heat capacity of 873 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 1,8-octanediol burned (kJ/mol). C3H1802(s) + 23/2 O2(g) –→8 CO2(g) + 9 H20(1) ΔΕ- kJ/mol
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