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@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

@X@user.full_name@X@ @GMU: What is the fraction of A remaining after 52.798 minutes if the first order rate constant is 3.680e-4 s-1?

@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 1.67e-8?4C2H2(g) + 5 H2(g) → C8H18(g) ΔGo = -819.870 kJ.

@X@user.full_name@X@ @GMU: What is the rate of consumption of A (M/s), if the rate of consumption of B is 0.381 M/s? Use the reaction below:3A + 4B + 5C → products

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3421 M A, 0.2341 M B, and 0.1120 M C. Which change will cause the equilibrium to shift from right to left if the reaction is exothermic? Use the reaction below.4A(aq) → 4 B(aq) +3 C(aq) K = 1.003