Chemistry, 16.04.2020 21:36, rogersdeloris1ovgm3b
Given that the standard free energies of formation (∆Gof) of Ag+(aq), Cl−(aq), and AgCl(s) are 77.1 kJ/mol, −131.2 kJ/mol, and −109.8 kJ/mol, respectively, calculate the solubility product, Ksp, for AgCl at 298 K. Hints: Calculate ∆Go first. and The reaction is: AgCl(s) ⇆ Ag+(aq) + Cl−(aq) Group of answer choices
Answers: 1
Chemistry, 21.06.2019 17:10, PSBSolarYT
For which one of the following reactions is the value of δh° rxn equal to δh° f for the product? a. 2 h2 (g) + o2 (g) → 2 h2o (l) b. n2 (g) + o2 (g) → 2 no (g) c. 2 h2 (g) + o2 (g) → 2 h2o (g) d. h2o (l) + 1/2 o2 (g) → h2o2 (l) e. none of the above
Answers: 1
Chemistry, 22.06.2019 04:30, ajsoccer1705
Using the periodic table, complete the table to describe each atom. type in your answers
Answers: 3
Given that the standard free energies of formation (∆Gof) of Ag+(aq), Cl−(aq), and AgCl(s) are 77.1...
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