For the reaction, `C+O_(2)rarrCO_(2)`, `DeltaH=-393 J`
`2Zn+O_(2) rarr 2ZnO`, `DeltaH=-412J`

Options

A. Carbon can oxidise `Zn`
B. Oxidation of carbon is not feasible
C. Oxidation of `Zn` is not fesible
D. `Zn` can oxidise carbon

Explanation

To solve the problem, we need to analyze the given reactions and their enthalpy changes (ΔH). The reactions provided are:

1. \( C + O_2 \rightarrow CO_2 \) with \( \Delta H = -393 \, \text{J} \)
2. \( 2Zn + O_2 \rightarrow 2ZnO \) with \( \Delta H = -412 \, \text{J} \)

We need to determine the feasibility of the reactions and whether carbon can oxidize zinc or vice versa.

### Step-by-Step Solution:

**Step 1: Understand the reactions and their enthalpy changes.**
- The negative ΔH values indicate that both reactions are exothermic, meaning they release energy.

**Step 2: Determine the reverse reaction for carbon.**
- If carbon is oxidizing zinc, we need to consider the reduction of carbon:
\[ CO_2 \rightarrow C + O_2 \]
- The ΔH for this reverse reaction will be the opposite of the forward reaction:
\[ \Delta H = +393 \, \text{J} \]

**Step 3: Calculate the ΔH for the oxidation of zinc.**
- The reaction for the oxidation of zinc is:
\[ Zn + \frac{1}{2} O_2 \rightarrow ZnO \]
- The ΔH for this reaction (from the second reaction) is:
\[ \Delta H = -206 \, \text{J} \quad \text{(since 2 moles are given, we divide by 2)} \]

**Step 4: Analyze the feasibility of carbon oxidizing zinc.**
- For carbon to oxidize zinc, the overall reaction must have a negative ΔH:
\[ \Delta H_{\text{overall}} = \Delta H_{\text{oxidation of carbon}} + \Delta H_{\text{oxidation of zinc}} \]
- Substituting the values:
\[ \Delta H_{\text{overall}} = 393 \, \text{J} - 206 \, \text{J} = 187 \, \text{J} \]
- Since 187 J is positive, carbon cannot oxidize zinc.

**Step 5: Determine the feasibility of zinc oxidizing carbon.**
- For zinc to oxidize carbon, we consider the reduction of zinc:
\[ ZnO \rightarrow Zn + \frac{1}{2} O_2 \]
- The ΔH for this reverse reaction is:
\[ \Delta H = +206 \, \text{J} \]
- Now, we need to consider the overall reaction:
\[ \Delta H_{\text{overall}} = \Delta H_{\text{oxidation of zinc}} + \Delta H_{\text{oxidation of carbon}} \]
- Substituting the values:
\[ \Delta H_{\text{overall}} = 206 \, \text{J} - 393 \, \text{J} = -187 \, \text{J} \]
- Since -187 J is negative, zinc can oxidize carbon.

### Conclusion:
- **Carbon cannot oxidize zinc.**
- **Zinc can oxidize carbon.**