@X@user.full_name@X@ @GMU: What is the freezing point when 12.47 g of Fe(NO3)3 (formula mass = 241.85 g/mol) is dissolved in 193.88 g H2O? The freezing point depression constant is 1.8600 (°C*kg)/mol. Assume any salt is completely ionic!

@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?SO2Cl2(g)→SO2(g) + Cl2(g)

@X@user.full_name@X@ @GMU: The reaction below is a exothermic reaction. What would one have to do to shift the equilibrium to the right?2NO2(g)→N2O4(g)

@X@user.full_name@X@ @GMU: What is the boiling point elevation when 12.98 g of K3PO4 (formula mass = 212.30 g/mol) is dissolved in 190.63 g H2O? The boiling point elevation constant is 0.5100 (°C*kg)/mol. Assume any salt is completely ionic!

@X@user.full_name@X@ @GMU: What is the value of Kc at 726.85 °C for the reaction below if Kp is 25.5886 at this temperature?H2(g) + CH4(g) → CO(g) + 3H2(g)

@X@user.full_name@X@ @GMU: Determine the mole fraction of toluene if 6.1017 g of toluene, C7H8, was mixed with 7.48 g of cyclohexene, C6H10. MW(C7H8) = 92.141 g/mol; MW(C6H10) = 82.145 g/mol.

@X@user.full_name@X@ @GMU: What is the molality of a solution made by combining 3.0988 g rubidium chloride, RbCl, with 0.2986 L of water (assume a density of 1.00 g/mL)? The molecular weight is 120.9205 g/mol.

@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 0.289 0.300 2.10e-7 0.483 0.300 4.54e-7 0.289 0.552 3.87e-7

@X@user.full_name@X@ @GMU: Determine the rate of consumption of I− if the rate for formation of I2 is 0.333 M/s. Use the reaction below.IO3− + 5I− + 6H+ → 3I2 + 3H2O

@X@user.full_name@X@ @GMU: Determine the rate of formation of I3− if the rate for formation of SO42− is 0.400 M/s. Use the reaction below.3I−(aq)+ S2O82−(aq) → I3−(aq) + 2SO42−(aq)