Blog

Calculate ΔSsurr at 298 K. 2NO2(g) → N2(g) + 2O2(g) ΔH = -66.4 kJ

A certain reaction has an activation energy of 25.0 kJ/mol. At what temperature will the reaction proceed three times faster than it did at 298 K?

Which of the following set of acids and conjugate bases would buffer most effectively at pH = 7.00?

Which of the following is true when ∆G = 0?

Calculate the pH of a buffer containing 1.25 M formic acid, HCOOH (Ka = 1.8 × 10-4) and 2.50 M sodium formate, HCOONa.You must show all of your work for credit.

For a certain reaction at 330 K, ∆Hsys = -9.9 kJ and ∆Ssys = 85 J/K, calculate ∆Suniv.

Calculate the pH of a solution with a hydroxide ion concentration of 5.25

For a certain reaction at 330 K, ∆Hsys = 9.9 kJ and ∆Ssys = 85 J/K, calculate ∆Suniv.

Calculate ΔG°rxn for the following reaction at 298 K. 2KCl(s)  → 2K(s) + Cl2(g)  ΔH° = 873 kJ;  ΔS° = 187 J/K Answer: ΔG°rxn  = [a] kJ

Predict the sign (∆S > 0 or ∆S < 0) of the entropy change (∆S) for the following processes. (a) CO2(s) ⟶ CO2(g)[c] (b) CaCO3(s) ⟶ CaO(s) + CO2(g) [d] (c) 4Fe(s) + 3O2(g) ⟶ 2Fe2O3(s) [e]