____________ predicts whether flow is laminar or turbulent.  

What is the molar solubility (in M) of manganese (II) hydroxide, Mn(OH)2, in water? Hint:  Ksp of Mn(OH)₂ is 2.1 × 10-13  

Given the standard reduction potentials below:  Half Reaction E° red (V) Ag+ (aq)  + e–  →  Ag (s)  +0.80 Fe3+ (aq)  +   e–  → Fe2+ (aq)   +0.77 Cu2+ (aq)  + 2 e–  → Cu (s)    +0.34 Sn4+ (aq) + 2 e–  → Sn2+ (aq)   +0.15 2H+ (aq) + 2 e–  →  H2 (g)  0.00 Pb2+ (aq) + 2 e –  → Pb (s)  –0.13 Sn2+ (aq)  +  2 e–  → Sn (s)  –0.14 Ni2+ (aq) + 2 e –  → Ni (s)   –0.28 Cd2+ (aq) + 2 e –  → Cd (s)   –0.40 Fe2+ (aq) + 2 e –  → Fe (s) –0.44 Cr3+ (aq) + 3 e– →  Cr (s)      –0.74 Zn2+ (aq) + 2 e –  → Zn (s)  –0.76 Al3+ (aq) + 3 e– →  Al (s) –1.66   Which of the following  substances would be the weakest reducing agent?

Consider the following voltaic cell with the overall cell reaction: Zn (s)   +   2 H+ (g)  ⟶ Zn2+ (g)   +    H2 (g) If the pressure of H2 gas is increased in the cathode cell, the value of Q will                  and the value of Ecell will                   .

At 25°C, the pH of a solution is 5.41.  What is the hydroxide ion concentration, , of this solution?  

Consider the following voltaic cell with the overall cell reaction: Zn (s)   +   2 H+ (g)  ⟶ Zn2+ (g)   +    H2 (g) If the pressure of H2 gas is decreased in the cathode cell, the value of Q will                  and the value of Ecell will                   .

Complete and balance the following redox half-reaction equation under acidic conditions.     Cr3+(s)   →   CrO42-(aq)       (acidic solution) How many electrons are transfered in this half-reaction when the equation is balanced using the set of smallest whole-number coefficients? 

Consider the following titration curve graphs:   Which plot shows the pH curve expected when NH3 is titrated by HNO3 ?

What is the molar solubility (in M) of iron (II) hydroxide, Fe(OH)2, in water? Hint:  Ksp of Fe(OH)₂ is 1.8 × 10-15

An example of a reaction that experiences a decrease in entropy, ΔS < 0, yet is spontaneous because of the release of a large quantity of heat, ΔH = −151 kJ, is the formation of solid ammonium nitrate from the reaction of gaseous nitric acid with gaseous ammonia.                        HNO3(g)   +   NH3(g)   →  NH4NO3 (s) The change in free energy under standard condition is: ΔG° =  −93. kJ/mol.  Calculate the equilibrium constant, K, for the reaction at T = 298 K.