@X@user.full_name@X@ @GMU: Hydrogen iodide decomposes at 410°C according to second order kinetics (see reaction below). The half-life for this reaction was measured to be 6.83e3 s when the initial concentration of HI was 4.75e-3 M. What is the rate constant for this reaction?HI(g) → H2(g) + I2(g)

@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 1.43e-6?4C2H2(g) + H2(g) → C8H10(g) ΔGo = -706.560 kJ.

@X@user.full_name@X@  @GMU: What is Kp for the reaction below, if Kc = 3.28e-3 at 305.4°C?3A(s) + 2B(g) → 3C(g)

@X@user.full_name@X@ @GMU: What would the [OH-] be after addition of 5.88 mL of 0.1000 M NaOH to 25.00 mL of 0.1000 HA (a weak acid, Ka = 3.32e-5)?

@X@user.full_name@X@ @GMU: The pH of a solution of HClO4 was 4.941. What was the hydronium ion concentration?

@X@user.full_name@X@ @GMU: What is the standard free energy change for the following cell?2Cu+(aq) + Sn(s) → 2Cu(s) + Sn2+(aq) Ecoell = 0.660V

@X@user.full_name@X@ @GMU: What is the pOH of a 0.1768 M H2CO3 ? See reaction belowH2CO3 + H2O → HCO-3 + H3O+ Ka = 4.300×10-7

@X@user.full_name@X@ @GMU: What is the conjugate base and base dissociation constant of NH+4 if its acid dissociation constant is 5.600×10-10 ?

John Schreifels @GMU: What is the total entropy change at 25oC for the reaction below, if the standard entropies of reactants and products are So(C(gr)) = 5.74 J/mol*K, So (H2(g)) = 130.68 J/mol*K, and So (C7H16(g)) = 426.3000J/mol*K and the heat of formation of C7H16(g)) is -187.9000 kJ/mol.C7H16(g) → 7C(gr) + 8H2(g)

@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 (C5H10(g)) = 347.7700J/mol*K and the heat of formation of C5H10(g)) is -20.9300 kJ/mol?C5H10(g) → 5C(gr) + 5H2(g)