The document provides instructions for calculating the standard cell potential for half-cell reactions and determining if redox reactions will occur spontaneously. It outlines 5 steps: 1) Identify oxidized and reduced ions, 2) Use table 21.2 to identify half-reactions, 3) Use the table to find reduction potentials, 4) Use the formula Reduction ion - Oxidized ion, 5) Plug in potentials to get the result. If the result is positive, the redox reaction will occur spontaneously. It concludes by listing 3 practice redox reactions.

1. Matthew Hunt 21.2
Chemistry

2. Calculating the Standard Cell
Potential for Half-Cells
Zn(s) + 2Ag+(aq)Zn2+(aq) + 2Ag(s)
1.) Figure out which ions are oxidized and which are reduced.
2.) Use the hand-dandy table 21.2 on page 740 to identify the
half-reactions
3.) Use the same table to find out the reduction potentials for
the ions
4.) Remember the formula: Reduction ion – Oxidized ion
5.) Plug in the reduction potentials in their place and add for
the final result

3. Determine if a Redox Reaction
Will Occur Spontaneously
 Zn(s) + 2Ag+(aq)Zn2+(aq) + 2Ag(s)
 If the previous result from the previous equation yields
a positive number, then the Redox Reaction will occur
spontaneously.
 Now try the practice problems on the handout sheet.

4. Mg(s) + Ni2+(aq)Mg2+(aq)+Ni(s)

5. Cu2+(aq)+Pb(s)Cu(s)+Pb2+(aq)

6. 2Ag+(aq)+Cr(s)2Ag(s)+Cr2+(aq)