Statement 1 Copper liberates hydrogen from a dilute solution of hydrochloric acid
Statement 2 `E^(@)` of Cu is higher than of `H_(2)`

Options

A. Statement 1 is true statement 2 is true , statement 2 is a corrrect explanation for statement 1
B. Statement 1 is true statement 2 is true statement 2 is not a correct explanation for statement 1
C. Statement 1 is true statement 2 is false
D. Statement 1 is false statement 2 is true

Explanation

To analyze the statements provided in the question, we need to evaluate each statement based on our understanding of redox reactions and the reactivity series.

### Step-by-Step Solution:

**Step 1: Evaluate Statement 1**
- The first statement claims that copper liberates hydrogen from a dilute solution of hydrochloric acid (HCl).
- To determine if this is true, we need to refer to the reactivity series of metals. In the reactivity series, metals are arranged in order of their ability to displace other metals from solutions of their ions.
- Copper (Cu) is less reactive than hydrogen (H). This means that copper cannot displace hydrogen from hydrochloric acid.
- Therefore, Statement 1 is **false**.

**Step 2: Evaluate Statement 2**
- The second statement claims that the standard electrode potential (E°) of copper is higher than that of hydrogen.
- The standard electrode potential for copper (Cu²⁺ + 2e⁻ → Cu) is +0.34 V, while for hydrogen (2H⁺ + 2e⁻ → H₂) it is defined as 0.00 V (standard reference).
- Since +0.34 V is indeed higher than 0.00 V, this indicates that copper has a higher reduction potential than hydrogen.
- Therefore, Statement 2 is **true**.

**Step 3: Conclusion**
- Based on the evaluations, we conclude that:
- Statement 1 is **false**.
- Statement 2 is **true**.

### Final Answer:
- Statement 1: False
- Statement 2: True