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@X@user.full_name@X@ @GMU: Determine the rate of formation of NO2 if the rate for formation of O2 is 0.299 M/s. Use the reaction below.2N2O5(g) → 4NO2(g) + O2(g)

@X@user.full_name@X@ @GMU: What is the solubility in mol/L of CO at a partial pressure of 296.4 torr, if the solubility at a partial pressure of 401.3 torr is 0.0005491 mol/L?

@X@user.full_name@X@ @GMU: Determine the rate of formation of NO2 if the rate for consumption of N2O5 is 0.309 M/s. Use the reaction below.2N2O5(g) → 4NO2(g) + O2(g)

@X@user.full_name@X@ @GMU: The following data was obtained by the method of initial rates. What is the rate law for the reaction of A with B to produce product? [A]o [B]o Rate, M/s 0.291 0.268 2.98e-6 0.441 0.268 2.98e-6 0.291 0.517 1.11e-5

@X@user.full_name@X@ @GMU: What is the molality of a solution made by combining 3.8135 g rubidium chloride, RbCl, with 0.3072 L of water (assume a density of 1.00 g/mL)? The molecular weight is 120.9205 g/mol.

John Schreifels @GMU: Determine the mass of LiCl required to produce a 0.2196 molal solution by dissolving LiCl in 176.7113 g of H2O. MW(LiCl) = 42.394 g/mol. 

@X@user.full_name@X@ @GMU: How many grams of potassium chloride, KCl, would be required to prepare a 0.1175 m KCl solution by combining this compound with 0.4495 L of water (assume a density of 1.00 g/mL)? The molecular weight is 74.551 g/mol.

What would be the expected rate law for the mechanism described below?1 H2O2 + I- → H2O + IO- slow 2 IO- + H2O2 → H2O + O2 + I- fast

@X@user.full_name@X@ @GMU: Determine the mole fraction of toluene if 6.5876 g of toluene, C7H8, was mixed with 9.96 g of benzene, C6H6. MW(C7H8) = 92.141 g/mol; MW(C6H6) = 78.114 g/mol.

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.1797 M A, 0.3333 M B, and 0.1797 M C. Which change will cause Qc to be less than Kc? Use the reaction below.6A → 3 B +3 C Kc = 0.432