For the reaction I2(s) + Cl2(g) → 2 ICl(g) ΔH° = 36 kJ and ΔS° = 158.8 J/K at 25 °C. Calculate ΔG° for the process at 25 °C.

What is the resulting pH after 1.00 mL of 1.00 M NaOH(aq) is added to 100. mL of a solution containing 0.18 M NH3(aq) and 0.10 M NH4Cl(aq)?  Kb of NH3 = 1.8 × 10−5 Enter your answer numerically and to two decimal places

Consider the hydrogen fuel cell reaction below at 298K. Given the following information, calculate the

The molar solubility of Cu(OH)2 (Ksp = 2.2 × 10−20) in a buffered solution with pH = 9.20 is closest to

For the reaction: I2 (s) + Cl2 (g) → 2 ICl (g) ΔH° = 36 kJ and ΔS° = 158.8 J/K at 25°C. Calculate the temperature at which Keq is 4.0 × 103. 

What can be concluded about the equilibrium constant, K, for a reaction if ∆G˚ is positive?

The heat of vaporization, ΔHvap of ethyl acetate (C4H8O2) is 35.1kJ/mol. Calculate the change in entropy ΔS in kJ/K, when 643.g of ethyl acetate boils at 77.1°C. Enter your numeric answer, without units, to 3 significant figures.

Which of the following act as buffer solutions? Select all that apply

What is the free Cu2+ concentration if 100.0 mL of 0.020 M Cu2+ solution is mixed with 100.0 mL of 4.0 M NH3? Kf for 2+ is 1.1 × 1013.

The titration curve below describes the: