@X@user.full_name@X@ @GMU: What is the solubility in mol/L of C2H6 at a partial pressure of 627.3 torr, if the solubility at a partial pressure of 517.8 torr is 0.001226 mol/L?

@X@user.full_name@X@ @GMU: What is the boiling point when 13.91 g of NaClO4 (formula mass = 122.44 g/mol) is dissolved in 171.40 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: A mixture containing an initial concentration of 0.1214 M for H2 and 0.0878 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

What would be the expected rate law for the mechanism described below?1 NO + 1/2O2 → NO2 fast 2 NO2 + SO2 → NO + SO3 slow

@X@user.full_name@X@ @GMU: Determine the rate of consumption of H2 if the initial concentration of N2 was 0.4216 M and decreased to 0.3132 M after 0.3305 hours. Use the reaction below.N2(g) + 3 H2(g) → 2NH3(g)

@X@user.full_name@X@ @GMU: What is the rate constant at 46.61°C for the reaction below if the rate constant is 3.70e-5 s-1 at 25.00°C and the activation energy is 104.00 kJ/mol?2N2O5(g)→ 4NO2(g) + O2(g)

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1738 M for H2 and 0.1430 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: When 2.785 g of urea was dissolved in 108.5 g of benzene, the freezing point was 276.5 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: Initially there were equilibrium concentrations of 0.1387 M A, 0.5000 M B, and 0.1387 M C. Which change will cause Qc to be greater than Kc? Use the reaction below.5A → 2 B +3 C Kc = 1.075

@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!