At `1000^(@)C`,
`Zn_((s)) +(1)/(2)O_(2(g)) to ZnO_((s)), DeltaG^(@)=-360 KJ "mol"^(-1)`
`C_((s)) + (1)/(2)O_(2(g)) to CO_((g)),DeltaG^(@) =-460 KJ "mol"^(-1)`
The correct statement is

Options

A. zinc can be oxidised by carbon monoxide
B. zince blend is produced during the reaction
C. zinc oxide can be reduced by graphite
D. zinc can be oxidised by graphite

Answer

To solve the given question, we will analyze the provided reactions and their Gibbs free energy changes (ΔG°).

### Step-by-Step Solution:

1. **Identify the Reactions and Their ΔG° Values:**
- Reaction 1: \( \text{Zn}_{(s)} + \frac{1}{2} \text{O}_{2(g)} \rightarrow \text{ZnO}_{(s)} \) with \( \Delta G° = -360 \, \text{kJ/mol} \)
- Reaction 2: \( \text{C}_{(s)} + \frac{1}{2} \text{O}_{2(g)} \rightarrow \text{CO}_{(g)} \) with \( \Delta G° = -460 \, \text{kJ/mol} \)

2. **Determine Spontaneity of the Reactions:**
- A negative ΔG° indicates that a reaction is spontaneous. Both reactions have negative ΔG° values, meaning both are spontaneous at 1000°C.

3. **Compare the ΔG° Values:**
- The ΔG° for the formation of CO (-460 kJ/mol) is more negative than that for the formation of ZnO (-360 kJ/mol). This indicates that the formation of CO is more thermodynamically favorable than the formation of ZnO.

4. **Consider the Reduction of ZnO:**
- Since the formation of CO is more favorable, we can use carbon (C) to reduce zinc oxide (ZnO). The reduction reaction can be represented as:
\[ \text{ZnO}_{(s)} + \text{C}_{(s)} \rightarrow \text{Zn}_{(s)} + \text{CO}_{(g)} \]
- This reaction is feasible because the oxidation of carbon (from C to CO) is favored.

5. **Conclusion:**
- Therefore, we conclude that zinc oxide can be reduced by carbon at 1000°C, making the correct statement: "Zinc oxide can be reduced by graphite."

### Final Answer:
The correct statement is: "Zinc oxide can be reduced by graphite."