@X@user.full_name@X@ @GMU: For a galvanic cell, the cathode has a ____ sign and is the site of ____.

@X@user.full_name@X@ @GMU: The cell potential was -0.773 V at 25oC and a Cu+(aq) concentration of 0.103 M. What was the pH of the solution? The H2(g) pressure was 1 atm at 25oC.2H+(aq) + 2Cu(s) → 2Cu+(aq) + H2(g) Ecoell = -0.5200 V

@X@user.full_name@X@ @GMU: What is the pOH of a 0.1275 M HNO2 ? See reaction belowHNO2 + H2O → NO-2 + H3O+ Ka = 4.600×10-4

@X@user.full_name@X@ @GMU: How much time in days would it take for a 1.9910 g sample of 14C to decay to a mass of 0.7346 g if it has a half-life of 1.807e11 s.

@X@user.full_name@X@ @GMU: By how much would the rate of reaction (see below) change if the concentration of H+ increased by a factor of 1.584. The rate law of this reaction is Rate = k2.BrO3- + 5Br- + 6H+ → 3Br2 + 3H2O

@X@user.full_name@X@ @GMU: By how much would the rate of reaction (see below) change if the concentration of CH3CHO increased by a factor of 1.542. The rate law of this reaction is Rate = k3/2.CH3CHO(g) → CH4(g) + CO(g)

@X@user.full_name@X@ @GMU: Calculate the of 108.32 mL of a buffer initially consisting of 0.1881 M CH3(CH2)2CH2NH2 and 0.0979 M CH3(CH2)2CH2NH3Cl after addition of 0.0028 mol of HCl. Assume that no volume change occurs after addition of the acid. The Kb of CH3(CH2)2CH2NH2 is 4.10e-4

@X@user.full_name@X@ @GMU: What is the pH of 3.22e-3 M HClO3 ?

@X@user.full_name@X@ @GMU: NO2 at 383°C decomposes to form NO and O2 according to second order kinetics (see reaction below). The half-life for this reaction was measured to be 3.46e1 s when the initial concentration of NO2 was 6.03e-3 M. What is the rate constant for this reaction?2NO2(g) → 2NO(g) + O2(g)

@X@user.full_name@X@ @GMU: What is the balanced reaction at the anode for the following galvanic cell?Cd(s) | Cd2+(aq) || Cu2+(aq) | Cu(s)