@X@user.full_name@X@ @GMU: How many grams of potassium hydroxide, KOH, would be required to prepare a 0.2434 m KOH solution by combining this compound with 0.3947 L of water (assume a density of 1.00 g/mL)? The molecular weight is 56.1056 g/mol.

@X@user.full_name@X@ @GMU: How many grams of rubidium chloride, RbCl, would be required to prepare a 0.1445 m RbCl solution by combining this compound with 0.3458 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: When 11.19 g of glucose was dissolved in 104.8 g of benzene, the freezing point was 275.6 K. What is the formula mass of this compound? The freezing point depression constant for benzene is 5.12 (°C*kg)/mol. The melting point and boiling points are 5.50°C and 80.10°C, respectively.

@X@user.full_name@X@ @GMU: How many grams of sodium hydroxide, NaOH, would be required to prepare a 0.1536 m NaOH solution by combining this compound with 0.3007 L of water (assume a density of 1.00 g/mL)? The molecular weight is 39.9971 g/mol.

@X@user.full_name@X@ @GMU: A possible reaction mechanism for the reaction between nitric oxide and bromine is shown below. Which species listed below is an intermediate? (1) NO(g) + Br2(g) → NOBr2(g) Slow, rate determining (2) NO(g) + NOBr2(g) → 2NOBr(g) Fast, equilibrium

@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.