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@X@user.full_name@X@ @GMU: What is the value of Ksp in water, if 8.20e-7 M of A2B3 dissolves according to the reaction below?A2B3(s)→2A(aq) + 3B(aq) where A and B are ions

@X@user.full_name@X@ @GMU: Which of the answers below is the correct representation according to the shorthand method of the following galvanic cell?Cu2+(aq) + Ni(s) → Cu(s) + Ni2+(aq)

@X@user.full_name@X@ @GMU: What is the rate of consumption of B (M/s), if the rate of consumption of C is 0.396 M/s? Use the reaction below:2A + 3B + 5C → products

@X@user.full_name@X@ @GMU: To what temperature would the reaction below need to be heated to have a rate constant of 9.46e-4 M-1s-1 if the rate constant was 2.700e-4 M-1s-1 at 327.00°C and the activation energy was 166.00 kJ/mol?H2(g) + I2(g) → 2HI(g)

@X@user.full_name@X@ @GMU: What is the value of Ksp in water, if 2.77e-7 M of A3B2 dissolves according to the reaction below?A3B2(s)→3A(aq) + 2B(aq) where A and B are ions

@X@user.full_name@X@ @GMU: What is the pOH of 5.60e-3 M HCl?

John Schreifels @GMU: What is the balanced reaction at the anode for the following galvanic cell?Sn(s) | Sn2+(aq) || Cu+(aq) | Cu(s)

@X@user.full_name@X@ @GMU: Calculate the [H3O+] of 118.28 mL of a buffer initially consisting of 0.1476 M NH2OH and 0.1728 M NH3OHBr after addition of 0.0033 mol of HCl. Assume that no volume change occurs after addition of the acid. The Kb of NH2OH is 9.10e-9

John Schreifels @GMU: Which reaction below would result in a net increase in entropy?

@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 (C4H6(g)) = 283.4000J/mol*K and the heat of formation of C4H6(g)) is 148.0700 kJ/mol?4C(gr) + 3H2(g) → C4H6(g)