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Consider the voltaic cell diagram:  Sn(s) | Sn2⁺(aq) || Ag⁺ (aq) | Ag (s) What is the standard cell potential, E°cell, (in V) for this voltaic cell? Hint: Refer to the table of standard reduction potentials provided. 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  

The combustion of ammonia proceeds by the reaction           4 NH3    +    7 O2  →  4 NO2    +    6 H2O When the rate of appearance of H2O is 1.10 Ms-1, the rate of disappearance of O2 is          Ms-1

A sample of sodium bicarbonate, NaHCO3,  is placed in a closed 1.0 L vessel at 398 K and allowed to decompose unil it reaches equilibrium according to the following equation:                                         2 NaHCO3 (s)   ⇌  Na2CO3(s) +  H2O (g)   +  CO (g)      Kp = 0.450 What is the partial pressure of CO (in atm)  at equilibrium?

Phophorous-32 decays by beta emission to form sulfur-32.   (In case the picture does not show: The picture indicated that 24 P-32 decayed to 3 P-32 in 9min. )  What is the decay constant, k, for P-32?

The following hypothetical reaction is zero order in A, second order in B, and first order in C: A +  B +  C  → products What is the correct rate law and the overall order of this reaction?    

Given the Kc value for the following reaction at a particular temperature:                         SO2 (g) + ½ O2 (g) ⇋ SO3 (g)                  Kc = 9.75 What is the value of Kc for the new equilibrium below at the same temperature?                         2 SO3 (g) ⇋ 2 SO2 (g) + O2 (g)

Consider the following reaction:   BrO3⎻ (aq)   +  5 Br⎻(aq)  +  6 H+(aq)   →  Br2(aq)   +   H2O(l)     This reaction has the rate law:  

Given the equilibrium constant, Kc = 3.0 x 103 for the following reaction:           2 KCl (s)  +  3 O2(g)  ⇌  2 KClO3(s)  What is the concentration of O2 (in M) at equilibrium?

The rate constant for a particular second order reaction is k = 0.0152 M−1 s −1 at 35°C.  If the initial concentration of reactant is 3.25 M, what is the concentration after 4 minutes? Hint: Make sure all units agree! 

Which of the following authors is most associated with Gothic literature in early America?