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 18 min. )  What is the decay constant, k, for P-32?

Given the two following reduction half reactions: Al3+(aq) +   3e- →   Al(s)                        Eo = −1.650 V Cd2+(aq) +   2e- →   Cd(s)                      Eo = −0.400 V Calculate ΔGº (in kJ) for a Al/Cd voltaic cell. Hint:  Remembmol)er that a voltaic cell runs on a spontaneous redox reaction.  Hint: Make sure to determine the total moles of electrons transferred for the cell.

Consider the voltaic cell diagram:  Al (s) | Al3⁺(aq) || Ni2⁺ (aq) | Ni (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  

Consider the reaction of elemental bromine with elemental chlorine to make a bromochloride compound at 600 K:                                          Br2(g)  +  Cl2(g)   ⇌   2 BrCl(g)       KP = 81.0 A closed vessel at 600 K is charged with 1.20 atm of Br2(g) and 1.20 atm of Cl2(g) initially and allowed to reach equilibrium. What is the partial pressure of the BrCl (in atm) at that equilibrium?

Which of the following combinations, when mixed in equal concentrations in water, would result in a buffer solution?  

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 6 min. )  What is the decay constant, k, for P-32?

Given the Kc value for the following reaction at a particular temperature:                         SO2 (g) + ½ O2 (g) ⇋ SO3 (g)                  Kc = 4.45 What is the value of Kc for the new equilibrium below at the same temperature?                         2 SO3 (g) ⇋ 2 SO2 (g) + O2 (g)

For the following equilibrium CH4(g)  +   2 H2S(g)   ⇌   CS2(g)   +    4 H2(g) the equilibrium constant, K = 4.28 x 10−34 at 280.0 °C. Which of the following best describes the reaction at equilibrium?

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 = 0.650 What is the partial pressure of CO (in atm)  at equilibrium?

Methane gas can be produced by the reaction of solid carbon with hydrogen gas as follows                     C(s)   +   2 H2(g)  ⇌   CH4(g)         Kp =  0.50 A vessel containing carbon is sealed and injected initially with hydrogen to a partial pressure of 2.0 atm and with methane to a partial pressure of 2.0 atm. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium?