@X@user.full_name@X@ @GMU: Determine the rate of consumption of I− if the rate for formation of I2 is 0.261 M/s. Use the reaction below.IO3− + 5I− + 6H+ → 3I2 + 3H2O

Sulfuryl Chloride, SO2Cl2 decomposes in the gas phase according to first order kinetics. Determine half-life and the rate constant.SO2Cl2(g) → SO2(g) + Cl2(g)

@X@user.full_name@X@ @GMU: What is the solubility in g/L of Kr at a partial pressure of 268.1 torr, if the solubility at a partial pressure of 431.8 torr is 0.1328 g/L?

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1408 M for H2 and 0.1161 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: The reaction below is a exothermic reaction. What would one have to do to shift the equilibrium to the right?4NO(g) + 6H2O(g)→4NH3(g) + 5O2(g)

@X@user.full_name@X@ @GMU: Determine the mole fraction of cyclohexene if 6.8460 g of cyclohexene, C6H10, was mixed with 8.49 g of cyclopentene, C5H8. MW(C6H10) = 82.145 g/mol; MW(C5H8) = 68.119 g/mol.

@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.