What does a “shift to the left” refer to in a white blood cell differential?  

What is the most common cause of megaloblastic anemia?

Which anemia is associated with inflammation, elevated ferritin, and impaired iron mobilization?

Calculate the value of E°cell for, and identify the reducing agent in the following reaction:                      2Au(s) + 3Ca2+(aq) → 2Au3+(aq) + 3Ca(s) 

Consider the following equilibria: 2SO3(g) ⇌ 2SO2(g) + O2(g)  Kc = 2.3 × 10–72NO3(g) ⇌ 2NO2(g) + O2(g)  Kc = 1.4 × 10–3Calculate the equilibrium constant for the reactionSO2(g) + NO3(g) ⇌ SO3(g) + NO2(g).

At 2600 K, ΔG° = 775 kJ for the vaporization of boron carbide:                                                        B4C(s) ⇌ 4 B(g) + C(s)  Find ΔG and determine if the process is spontaneous if the reaction vessel contains 4.00 mol B4C(s), 0.400 mol of C(s), and B(g) at a partial pressure of 1.0 × 10-5 atm. 

Determine the nuclear stability of the 50Mn isotope. If it is radioactive, choose the most likely mode of decay.

Consider the 4– ion. Determine which responses are true statements. I. The oxidation number of Co is –2.II. The coordination number of cobalt is 6.III. It is paramagnetic.IV. It is a low-spin complex.

Use the tabulated half-cell reduction potentials to calculate the equilibrium constant, K, for the following balanced redox reaction at 25°C.                                             2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10-5 M in calcium ion and 4.75 × 10-5 M in oxalate ion.  What will happen once these solutions are mixed?  Ksp (CaC2O4) = 2.3 × 10-9