62. Solving a chemistry problem
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1. Calculate the enthalpy of hydration of sodium sulfate, if it is known that the enthalpy of the dissolution of anhydrous salt Na2SO4 (K) is -2.3 kJ/mol, the enthalp of the dissolution of crystallineratic
Na2SO4 10H2O (g) = Na2SO4*10H2O (K) ΔH1 =?
Na2SO4*10H2O (K) H2O (F) = Na2SO4 (P); ΔN2 = 78.6 kJ/mol
Na2SO4 (K) H2O (F) = Na2SO4 (P); ΔN3 = -2.3 kJ/mol
Na2SO4 10H2O (g) = Na2SO4*10H2O (K) ΔH1 =?
Na2SO4*10H2O (K) H2O (F) = Na2SO4 (P); ΔN2 = 78.6 kJ/mol
Na2SO4 (K) H2O (F) = Na2SO4 (P); ΔN3 = -2.3 kJ/mol
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- Content type File
- Content description 6,68 kB
- Updated on the site 30.12.2022
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If you do not open the file - install the RAR archiver. Inside the archive you will find a solution in Word format.
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