Chemistry Course Help with Heat of Dilution
7.10 Heat of Dilution
The amount of heat evolved or absorbed when solution containing one mole of solute is diluted from one concentration to another. For example,
HCl(g) + 10H2O ® HCl.10H2O; DH1 = – 69.01 kJ/mol
HCl(g) + 25H2O ® HCl.25H2O; DH2 = – 72.03 kJ/mol
HCl(g) + 40H2O ® HCl.40H2O; DH3 = – 72.79 kJ/mol
HCl(g) + ¥H2O ® HCl.¥H2O; DH¥ = – 74.85 kJ/mol
If we subtract first equation from the second in the above set, we get
HCl.10H2O + 15H2O ® HCl.25H2O; DH = (DH2 – DH1) = – 3.02 kJ/mol
This value of DH is the heat of dilution. The heat of dilution of a solution is dependent on the original concentration of the solution and on the amount of the solvent added.
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