@X@user.full_name@X@ @GMU: What is the cell voltage for the following cell?2Fe3+(aq) + 3Cd(s) → 2Fe(s) + 3Cd2+(aq) ΔGo = -208.408 kJ

@X@user.full_name@X@ @GMU: NO2 at 378°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 2.56e1 s when the initial concentration of NO2 was 9.54e-3 M. What is the rate constant for this reaction?2NO2(g) → 2NO(g) + O2(g)

@X@user.full_name@X@ @GMU: Which product in the reaction below is a base (this one first in the answer) and which product is an acid?ClO-4 + HClO → HClO4 + ClO-

@X@user.full_name@X@ @GMU: How much energy in kJ is released to form one mole of 204Pb from protons, electrons, and neutrons if the nucleus has a mass of 203.973020 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 cell voltage for the following cell?Fe3+(aq) + Al(s) → Fe(s) + Al3+(aq) ΔGo = -468.917 kJ

@X@user.full_name@X@ @GMU: By how much would the rate of reaction (see below) change if the concentration of CO increased by a factor of 2.304. The rate law of this reaction is Rate = k[NO2]2.NO2(g) + CO(g) → CO2(g) + NO(g)

@X@user.full_name@X@ @GMU: What is the solubility in g/L of SO2 at a partial pressure of 629.1 torr, if the solubility at a partial pressure of 495.1 torr is 61.61 g/L?

@X@user.full_name@X@ @GMU: To what temperature would you have to heat carbon disulfide, CS2,(l) to cause its vapor pressure to become 176.7 mm Hg if its heat of vaporization and boiling point are 26.80 kJ/mol and 319.1 K, respectively?

@X@user.full_name@X@ @GMU: When 0.3416 g of aspirin was dissolved in 106.5 mL of water, the osmotic pressure at 26.90°C was 0.4470 atm. What is the formula mass of this compound?

@X@user.full_name@X@ @GMU: What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C3H4(g)) = 248.2000J/mol*K and the heat of formation of C3H4(g)) is 185.5200 kJ/mol?3C(gr) + 2H2(g) → C3H4(g)