Question

1. Calculate the standard cell potential (from the Standard Reduction Potentials Table located in Files) for each reaction below, and note whether the reaction is spontaneous under standard state conditions. 1. Mg(s) + Ni2+(aq) --> Mg2+(aq) + Ni(s) 2. 2 Ag+(aq) + Cu(s) --> Cu2+(aq) + 2 Ag(s) 3. Mn(s) + Sn(NO3)2(aq) --> Mn(NO3)2(aq) + Sn(s) 4. 3 Fe(NO3)2(aq) + Au(NO3)3(aq) --> 3 Fe(NO3)3(aq) + Au(s) 2. Write the balanced cell reaction for the cell schematic below, calculate the standard cell potential, and note whether the reaction is spontaneous under standard state conditions. Cu(s) | Cu2+(aq) || Au3+(aq) | Au(s)

          1. Calculate the standard cell potential (from the Standard Reduction Potentials Table located in Files) for each reaction below, and note whether the reaction is spontaneous under standard state conditions.
1. Mg(s) + Ni2+(aq) --> Mg2+(aq) + Ni(s)
2. 2 Ag+(aq) + Cu(s) --> Cu2+(aq) + 2 Ag(s)
3. Mn(s) + Sn(NO3)2(aq) --> Mn(NO3)2(aq) + Sn(s)
4. 3 Fe(NO3)2(aq) + Au(NO3)3(aq) --> 3 Fe(NO3)3(aq) + Au(s)
2. Write the balanced cell reaction for the cell schematic below, calculate the standard cell potential, and note whether the reaction is spontaneous under standard state conditions.
Cu(s) | Cu2+(aq) || Au3+(aq) | Au(s)

1. Calculate the standard cell potential (from the Standard Reduction Potentials Table located in Files) for each reaction below, and note whether the reaction is spontaneous under standard state conditions.
1. Mg(s) + Ni2+(aq) –> Mg2+(aq) + Ni(s)
2. 2 Ag+(aq) + Cu(s) –> Cu2+(aq) + 2 Ag(s)
3. Mn(s) + Sn(NO3)2(aq) –> Mn(NO3)2(aq) + Sn(s)
4. 3 Fe(NO3)2(aq) + Au(NO3)3(aq) –> 3 Fe(NO3)3(aq) + Au(s)
2. Write the balanced cell reaction for the cell schematic below, calculate the standard cell potential, and note whether the reaction is spontaneous under standard state conditions.
Cu(s) | Cu2+(aq) || Au3+(aq) | Au(s)

Added by Cassie V.

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