Consider a solution made by mixing 500.0 mL of 4.0 M NH 3 and 500.0 mL of 0.40 M AgNO 3 . Ag + reacts with NH 3 to form AgNH 3 + and Ag(NH 3 ) 2 + : Ag + ( a q ) + N H 3 ( a q ) ⇌ A g N H 3 + ( a q ) K 1 = 2.1 × 10 3 AgNH 3 + ( a q ) + N H 3 ( a q ) ⇌ A g ( N H 3 ) 2 + ( a q ) K 2 = 8. 2 × 10 3 Determine the concentration of all species in solution.
Consider a solution made by mixing 500.0 mL of 4.0 M NH 3 and 500.0 mL of 0.40 M AgNO 3 . Ag + reacts with NH 3 to form AgNH 3 + and Ag(NH 3 ) 2 + : Ag + ( a q ) + N H 3 ( a q ) ⇌ A g N H 3 + ( a q ) K 1 = 2.1 × 10 3 AgNH 3 + ( a q ) + N H 3 ( a q ) ⇌ A g ( N H 3 ) 2 + ( a q ) K 2 = 8. 2 × 10 3 Determine the concentration of all species in solution.
Solution Summary: The author explains the solubility product of a substance's dissolved ion concentration raised to its power of its stoichiometric coefficients.
The standard Gibbs energies of formation of CaO(s), CaCO3 (calcite), and CO2 (g) are
-604.04, -1128.80, and -394.37 kJ/mol, respectively. Find the value of AG, and Keq for the
following reaction:
CaCO3 CaO (s) + CO2 (g)
[ap
A dry mixture containing 1 g of each solid [CaCO3(s) and CaO(s)] is on the lab bench in
contact with the atmosphere, which contains a partial pressure of 10-35 bar CO2 (g). What is
the total Gibbs free energy of the system containing all three species before any reaction has
happened? Does the equilibrium driving force favor conversion of one of the solids into the
other, or are the solids equilibrated with one another?
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