For the reaction,
`C+O_(2) rarr CO_(2), DeltaH=-393J`
`2Zn+O_(2) rarr 2ZnO,DeltaH=-412J`
Which one is correct ?

Options

A. Carbon can reduce `ZnO` to `Zn`
B. Oxidation of carbon is not feasible
C. Oxidation of `Zn` is not feasible
D. `Zn` liberates more heat than carbon during oxidation

Explanation

To analyze the reactions and determine which statements are correct, we will go through the information provided step by step.

### Step 1: Understand the Reactions and Their Enthalpy Changes
We have two reactions with their respective enthalpy changes (ΔH):
1. \( C + O_2 \rightarrow CO_2 \), \( \Delta H = -393 \, \text{J} \)
2. \( 2Zn + O_2 \rightarrow 2ZnO \), \( \Delta H = -412 \, \text{J} \)

### Step 2: Convert ΔH for the Second Reaction to Per Mole
The enthalpy change for the second reaction is given for 2 moles of Zn:
- For 1 mole of Zn, the ΔH will be:
\[ \Delta H = \frac{-412 \, \text{J}}{2} = -206 \, \text{J} \]

### Step 3: Analyze the Reduction of ZnO by Carbon
Next, we need to determine if carbon can reduce ZnO to Zn. The reduction reaction can be written as:
\[ ZnO + C \rightarrow Zn + CO \]
To find the ΔH for this reaction, we need to consider the enthalpy changes involved:
- The enthalpy of formation for ZnO is \( -206 \, \text{J} \) (for 1 mole).
- The enthalpy of formation for CO is \( -393 \, \text{J} \).

### Step 4: Calculate the Overall ΔH for the Reduction Reaction
Using Hess's law, we can find the ΔH for the reduction reaction:
\[ \Delta H = \Delta H_{ZnO} + \Delta H_{C} \]
Substituting the values:
\[ \Delta H = (-206 \, \text{J}) + (-393 \, \text{J}) = -599 \, \text{J} \]

### Step 5: Determine the Feasibility of the Reaction
Since the ΔH for the reduction of ZnO by carbon is negative (\(-599 \, \text{J}\)), this indicates that the reaction is exothermic and therefore feasible.

### Step 6: Analyze the Statements
1. **Carbon can reduce ZnO to Zn**: True, since the reaction is feasible.
2. **Oxidation of carbon is not feasible**: False, because the oxidation of carbon (to CO2) is feasible as ΔH is negative.
3. **Oxidation of zinc is not feasible**: False, because the oxidation of zinc (to ZnO) is also feasible as ΔH is negative.
4. **Zinc liberates more energy than carbon during oxidation**: False, because the energy released by the oxidation of carbon is greater than that of zinc when considering per mole.

### Conclusion
Based on the analysis, the correct statement is that carbon can reduce ZnO to Zn.

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