@X@user.full_name@X@ @GMU: When 0.3712 g of sucrose was dissolved in 107.1 mL of water, the osmotic pressure at 14.61°C was 0.2392 atm. What is the formula mass of this compound?

@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? o o Rate, M/s 0.258 0.322 2.16e-5 0.411 0.322 2.72e-5 0.258 0.526 2.16e-5

@X@user.full_name@X@ @GMU: Determine the rate of consumption of IO3− if the rate for consumption of I− is 0.273 M/s. Use the reaction below.IO3− + 5I− + 6H+ → 3I2 + 3H2O

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.2000 M for H2 and 0.1762 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: What is the rate constant at 447.21°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)

@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: What is the solubility in g/L of CH2CHCl at a partial pressure of 526.5 torr, if the solubility at a partial pressure of 427.7 torr is 3.201 g/L?

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1663 M for H2 and 0.1328 M for I2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HI?H2(g) + I2(g) → 2HI(g) Kc = 48.7000

@X@user.full_name@X@ @GMU: Determine the mole fraction of toluene if 7.1397 g of toluene, C7H8, was mixed with 6.86 g of benzene, C6H6. MW(C7H8) = 92.141 g/mol; MW(C6H6) = 78.114 g/mol.

@X@user.full_name@X@ @GMU: What is the boiling point elevation when 10.85 g of Co(NO3)3 (formula mass = 244.93 g/mol) is dissolved in 163.41 g H2O? The boiling point elevation constant is 0.5100 (°C*kg)/mol. Assume any salt is completely ionic!