Given `E_(Ag^(o+)|Ag)^(@) = + 0.80V , E_(Co^(2+)|Co)^(@) = -0.28 V, E_(Cu^(2+)|Cu)^(@) = + 0.34V, E_(Zn^(2+)|Zn)^@ = -0.76 V`
Which metal will corrode fastest?

Options

A. Ag
B. Cu
C. Co
D. Zn

Answer

To determine which metal will corrode the fastest among the given options, we need to analyze the standard reduction potentials (SRP) provided for each metal. The metal with the lowest standard reduction potential will corrode the fastest because it is the best reducing agent, meaning it is more likely to lose electrons (oxidize) in a corrosion reaction.

### Step-by-Step Solution:

1. **List the Standard Reduction Potentials:**
- \( E_{Ag^{+}/Ag} = +0.80 \, V \)
- \( E_{Co^{2+}/Co} = -0.28 \, V \)
- \( E_{Cu^{2+}/Cu} = +0.34 \, V \)
- \( E_{Zn^{2+}/Zn} = -0.76 \, V \)

2. **Identify the Most Negative Standard Reduction Potential:**
- Among the values, we need to find the one that is the most negative, as this indicates the strongest tendency to oxidize.
- The values are:
- \( +0.80 \, V \) (Ag)
- \( -0.28 \, V \) (Co)
- \( +0.34 \, V \) (Cu)
- \( -0.76 \, V \) (Zn)

3. **Compare the Values:**
- The most negative value is \( -0.76 \, V \) for zinc (Zn).
- The other values are higher (less negative) compared to zinc.

4. **Conclusion:**
- Since zinc has the lowest standard reduction potential, it will corrode the fastest among the metals listed.

### Final Answer:
**Zinc (Zn) will corrode the fastest.**