@X@user.full_name@X@ @GMU: How much time in minutes would it take for a 1.9957 g sample of 33P to decay to a mass of 1.1357 g if it has a half-life of 2.160e6 s.

@X@user.full_name@X@ @GMU: The osmotic pressure of a 15.060 mM solution of CaCl2 is 589.249 mm Hg at 29.76 °C. How many ions per formula unit of CaCl2 must there be? The compound may not be completely ionic.

@X@user.full_name@X@ @GMU: The osmotic pressure of a 14.019 mM solution of Fe(NO3)3 is 0.924 atm at 28.97 °C. How many ions per formula unit of Fe(NO3)3 must there be? The compound may not be completely ionic.

@X@user.full_name@X@ @GMU: What would the [H3O+] be after addition of 18.53 mL of 0.1000 M NaOH to 25.00 mL of 0.1000 HA (a weak acid, Ka = 6.66e-5)?

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3808 M A, 0.2234 M B, and 0.1185 M C. Which change will cause the equilibrium to shift from left to right if the reaction is exothermic? Use the reaction below.6A(aq) → 3B(aq) +2C(aq) K = 1.190

@X@user.full_name@X@ @GMU: What is the solubility in mol/L of CH3Br at a partial pressure of 289.4 torr, if the solubility at a partial pressure of 394.0 torr is 0.08244 mol/L?

@X@user.full_name@X@ @GMU: What is Kp for the reaction below, if Kc = 3.76e-5 at 170.9°C?4A(s) + 4B(g) → 2C(g)

@X@user.full_name@X@ @GMU: NaBr has a face-centered cubic unit cell in which the Br- anions occupy corners and face centers, while the cations fit into the hole between adjacent anions. What is the radius of Na+ if the ionic radius of Br- is 195.0 pm and the density of NaBr is 3.200 g/cm3?

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3867 M A, 0.2230 M B, and 0.1026 M C. Which change will cause the equilibrium to shift from right to left if the reaction is exothermic? Use the reaction below.5A(aq) → 2 B(aq) +2 C(aq) K = 0.661

@X@user.full_name@X@ @GMU: By how much would the rate of reaction (see below) change if the concentration of CO increased by a factor of 2.413. The rate law of this reaction is Rate = k[NO2]2.NO2(g) + CO(g) → CO2(g) + NO(g)