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@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 (C8H14(g)) = 446.3500J/mol*K and the heat of formation of C8H14(g)) is 82.4600 kJ/mol?C8H14(g) → 8C(gr) + 7H2(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)

@X@user.full_name@X@ @GMU: The osmotic pressure of an unknown solution is 1.424 atm at 30.85 °C. Which of the solutions below is the most likely one? Assume any salt is completely ionic!

@X@user.full_name@X@ @GMU: What is the value of Ksp in water, if 2.90e-8 M of A3B3 dissolves according to the reaction below?A3B3(s)→3A(aq) + 3B(aq) where A and B are ions

@X@user.full_name@X@ @GMU: What is the coefficient, b, in the reaction below, if Kc = 2.23e-3 and Kp = 0.0836 at 183.72°C?3A(s) + bB(g) → 4C(g)

@X@user.full_name@X@ @GMU: Which base listed below would be the best to creat a buffer having a pH of 10.9059?

@X@user.full_name@X@ @GMU: How much time in days would it take for a 1.7139 g sample of 14C to decay to a mass of 0.6940 g if it has a half-life of 1.807e11 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 5.40e1 s when the initial concentration of NO2 was 3.86e-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 cathode for the following galvanic cell?Cu(s)| Cu2+(aq) || Sn2+(aq) | Sn(s)

@X@user.full_name@X@ @GMU: What is the equilibrium concentration of H3O+ in 0.1321 M H2S? See reaction belowH2S + H2O → HS- + H3O+ Ka = 9.100×10-8