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@X@user.full_name@X@ @GMU: What is the rate of consumption of A (M/s), if the rate of consumption of C is 0.326 M/s? Use the reaction below:2A + 3B + 6C → products

@X@user.full_name@X@ @GMU: What is the value of Ksp in water, if 4.63e-6 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 balanced reaction at the anode for the following galvanic cell?Fe(s) | Fe3+(aq) || Sn2+(aq) | Sn(s)

@X@user.full_name@X@ @GMU: What is the pH of 1.58e-4 M H2SO4 ?

@X@user.full_name@X@ @GMU: Calculate the [H3O+] of 107.36 mL of a buffer initially consisting of 0.1513 M (CH3)3N and 0.1415 M (CH3)3NHBr after addition of 0.0030 mol of HCl. Assume that no volume change occurs after addition of the acid. The Kb of (CH3)3N is 6.30e-5

@X@user.full_name@X@ @GMU: What is the rate constant at 446.66°C for the reaction below if the rate constant is 1.30 M-1s-1 at 427.00°C and the activation energy is 134.00 kJ/mol?NO2(g) + CO(g) → NO(g) + CO2(g)

John Schreifels @GMU: To what temperature would the reaction below need to be heated to have a rate constant of 2.25 M-1s-1 if the rate constant was 1.300 M-1s-1 at 427.00°C and the activation energy was 134.00 kJ/mol?NO2(g) + CO(g) → NO(g) + CO2(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 2.394. The rate law of this reaction is Rate = k[BrO3-][Br-][H+]2.BrO3- + 5Br- + 6H+ → 3Br2 + 3H2O

@X@user.full_name@X@ @GMU: What is the correct expression for the solubility product of silver carbonate?Ag2CO3(s) → 2Ag+(aq) + CO32-(aq)

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