Enthalpy for the reaction `C+O_(2)rarrCO_(2)` is

Options

A. Positive
B. Negative
C. Zero
D. None

Explanation

To determine the enthalpy change for the reaction \( C + O_2 \rightarrow CO_2 \), we can follow these steps:

### Step 1: Identify the Reaction Type
The given reaction involves the combustion of carbon in the presence of oxygen to form carbon dioxide. This is a combustion reaction.

**Hint:** Combustion reactions typically involve a fuel (in this case, carbon) reacting with oxygen to produce heat and light.

### Step 2: Determine the Nature of the Reaction
Combustion reactions are generally exothermic, meaning they release heat. This is an important characteristic of the reaction we are analyzing.

**Hint:** Remember that exothermic reactions release energy, which is often observed as heat.

### Step 3: Understand Enthalpy Change (ΔH)
In thermodynamics, the change in enthalpy (ΔH) for an exothermic reaction is negative because energy is released to the surroundings.

**Hint:** For exothermic reactions, ΔH is negative, indicating that the products have lower energy than the reactants.

### Step 4: Conclusion on Enthalpy for the Reaction
Since the combustion of carbon is exothermic, we conclude that the enthalpy change for the reaction \( C + O_2 \rightarrow CO_2 \) is negative. Therefore, the correct representation of the enthalpy change is a negative value.

**Hint:** Look for options that indicate a negative ΔH when considering the enthalpy change for exothermic reactions.

### Final Answer
The enthalpy change for the reaction \( C + O_2 \rightarrow CO_2 \) is negative, indicating an exothermic reaction.