@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: 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: What is the pH of 3.22e-3 M HClO3 ?

@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: The osmotic pressure of a 17.490 mM solution of Na3PO4 is 951.569 mm Hg at 20.71 °C. How many ions per formula unit of Na3PO4 must there be? The compound may not be completely ionic.

@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)

@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: Determine the molality of a 5.664 wt % aqueous solution of NaF.

John Schreifels @GMU: What is the change in mass of 82Kr when it is formed from protons, electrons and neutrons if the atom has a mass of  81.913482 amu? The masses of the proton, electron and neutron are 1.00728 amu, 0.000549 amu and 1.00867 amu, respectively.

@X@user.full_name@X@ @GMU: What is the balanced reaction at the anode for the following galvanic cell?Cu(s) | Cu2+(aq) || Sn2+(aq) | Sn(s)