Summary:
- At equilibrium the for a reversible reaction is equal to zero.
- The natural logarithm of a number less than one is negative and so the sign of is positive.
- The large positive free energy change leads to a value that is extremely small.
- Both lead to the conclusion that the reactants are highly favored and very few product molecules are present at equilibrium.
- The solubility product constant of lead(II) iodide is 1.4 × 10-8 at 25°C.
Hmm...
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