The molar solubility of __________ is not affected by the pH of the solution.

For a process with ΔSsys < 0, which one of the following statements is correct? 

For a chemical reaction that is spontaneous in the reverse direction, it is found that ΔSsys > 0. This means ________

The reaction   4 Ag(s) + O2(g)  → 2 Ag2O(s) favors Ag2O at low temperature, but it favors Ag and O2 at high temperatures. How can this be explained in terms of ΔH and ΔS?   

Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 35oC. Predict whether or not this reaction will be spontaneous at this temperature. CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) ΔHorxn = -890.4 kJ

When a solution of DNA in water is heated (energy as heat is transferred), the double helix separates into two single strands. This process is called melting. What can be deduced from this information about the signs of the enthalpy and entropy changes for DNA melting?

Place the following in order of decreasing standard molar entropy. NaCl(g)            Na3PO4(aq)            NaCl(aq)

The reaction  Cr(en)33+(aq) + 6 NH3(aq) --> Cr(NH3)63+(aq) + 3en(aq)  where en represents ethylenediamine, is endothermic. What can possibly be true for the spontaneity of the reaction.

Which substance would have the largest standard molar entropy?

Consider the following balanced redox reaction Mn2+(aq) + S2O82-(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2SO42-(aq) Which of the following statements is true? 

3Ag2S(s) + 2Al(s) +6OH–(aq) --> 6Ag(s) + 2Al(OH)3(s) + 3S2–-(aq) For the above reaction would the Ecell increase  decrease or remain the same if a strong acid is added on the anode.

Consider the galvanic cell, Zn(s) ∣ Zn2+(aq) ∣∣ Pb2+(aq) ∣ Pb(s). Which one of the following changes to the cell would cause the cell potential to decrease (i.e., become Less positive)?

According to the standard reduction potentials Pb2+(aq) + 2e- → Pb(s) E˚= -0.12 V Fe2+(aq) + 2e- → Fe(s) E˚= -0.44 V Zn2+(aq) + 2e- → Zn(s) E˚= -0.76 V Which species will reduce Mn3+ to Mn2+ (E° = 1.51 V), but will NOT reduce Cr3+ to Cr2+ (E° = –0.40 V)?

In one episode of the 1960s television sitcom, Gilligan’s Island, the famous “professor” constructed voltaic cells to use as substitutes for their radio’s dead batteries. A single D-cell has an emf of 1.5 V. Which scraps of metal from their damaged boat, the Minnow, could best be used to create a 1.5 V voltaic cell? Assume that coconuts make great beakers and that seawater is a terrific electrolyte. Metal/Metal ion iron/iron(II) (the anchor) –0.44 V lead/lead(II) (fishing weights) –0.126 V silver/silver(I) (Mrs. Howell’s brooch) +0.799 V aluminum/aluminum(III) (the boat’s flagpole) –1.677 V

A voltaic cell prepared using zinc and iodine has the following line notation. Zn(s) | Zn2+(aq) || I2(s) | I-(aq) | C (graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

What is the shorthand notation that represents the following galvanic cell reaction?   2 Fe2+(aq) + Cl2(g) → 2 Fe3+(aq) + 2 Cl-(aq)