Write the oxidation half-reaction, the reduction half-reaction, and thecomplete reaction for the formation of calcium sulfide from the elements Ca and S.Remember, the electron gain must equal the electron loss.

Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Mn metal is put into a 1M aqueous Al3+ solution.If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.     +              +

1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -0.52 V (minus 0.52 V). 2.Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.46 volts.

Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.