@X@user.full_name@X@ @GMU: Determine the rate of consumption of I− if the initial concentration of IO3− was 0.6164 M and decreased to 0.5670 M after 0.2017 hours. Use the reaction below.IO3− + 5I− + 6H+ → 3I2 + 3H2O

@X@user.full_name@X@ @GMU: The osmotic pressure of an unknown solution is 0.321 atm at 33.94 °C. Which of the solutions below is the most likely one? Assume any salt is completely ionic!

Which of the following conditions will cause equilibrium to shift to the right?N2O5(g) ⇋ NO2(g)) + NO3(g)

@X@user.full_name@X@ @GMU: The reaction below is an endothermic reaction. What would one have to do to increase the size of the equilibrium constant?4NH3(g) + 5O2(g)→4NO(g) + 6H2O(g)

@X@user.full_name@X@ @GMU: What is the mole fraction of sodium sulphate, Na2SO4, in an aqueous solution that contains 1.2241 g of sodium sulphate dissolved in 25.1317 grams of water? MW(Na2SO4) = 142.043 g/mol.

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1987 M for H2 and 0.1540 M for Cl2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HCl?H2(g) + Cl2(g) → 2HCl(g) Kc = 5.00e16

@X@user.full_name@X@ @GMU: It took 389.6 s for 45.95% of a substance to react according to first-order kinetics. What is the value of the rate constant?

@X@user.full_name@X@ @GMU: What is the solubility in g/L of He at a partial pressure of 456.0 torr, if the solubility at a partial pressure of 342.1 torr is 0.0006667 g/L?

@X@user.full_name@X@ @GMU: Determine the molality of LiBr if 7.1501 g of LiBr was dissolved in 176.30 g of H2O. MW(LiBr) = 86.845 g/mol.

John Schreifels @GMU: Determine the mass of LiCl required to produce a 0.2309 molal solution by dissolving LiCl in 294.5576 g of H2O. MW(LiCl) = 42.394 g/mol.