Enter your answer in the provided box. Ksp for Co(OH)2 at 25°C is 3.3 × 10?16. Using this and data from your textbook, calculate the value of ?G o f for Co(OH)2(s). kJ/mol

88 kJ/mol

Explanation:

Let's consider the solution of Co(OH)₂.

Co(OH)₂(s) ⇄ Co²⁺(aq) + 2 OH⁻(aq)

The solubility product (Ksp) is 3.3 × 10⁻¹⁶. We can find the Gibbs free energy change (ΔG°) using the following expression.

ΔG° = - R × T × lnKsp

where,

R: ideal gas constant

T: absolute temperature (25°C + 273.15 = 298 K)

ΔG° = - R × T × lnKsp

ΔG° = - (8.314 × 10⁻³ kJ/mol.K) × 298 K × ln 3.3 × 10⁻¹⁶

ΔG° = 88 kJ/mol

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

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