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@X@user.full_name@X@ @GMU: What is the concentration of OH- in 0.1232 M H2CO3 ? See reaction belowH2CO3 + H2O → HCO-3 + H3O+ Ka = 4.300×10-7

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3387 M A, 0.2024 M B, and 0.1151 M C. Which change will cause the equilibrium to shift from left to right if the reaction is endothermic? Use the reaction below.5A(aq) → 3 B(aq) +2 C(aq) K = 0.999

@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: 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 (C7H14(g)) = 424.5800J/mol*K and the heat of formation of C7H14(g)) is -62.1600 kJ/mol?C7H14(g) → 7C(gr) + 7H2(g)

@X@user.full_name@X@ @GMU: How much time in minutes would it take for a 2.4869 g sample of 235U to decay to a mass of 1.7354 g if it has a half-life of 7.800e8 s.

@X@user.full_name@X@ @GMU: Which pair of substances are bases in the reaction below?ClO-4 + HClO → HClO4 + ClO-

@X@user.full_name@X@ @GMU: What is the pOH of 1.11e-3 M HCl?

@X@user.full_name@X@ @GMU: NO2 at 354°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 1.91e2 s when the initial concentration of NO2 was 2.91e-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 rate of consumption of C (M/s), if the rate of consumption of A is 0.225 M/s? Use the reaction below:4A + 5B + 6C → products

@X@user.full_name@X@ @GMU: What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 8.59e-6?2C2H2(g) + H2(g) → C4H6(g) ΔGo = -216.790 kJ.