Which of the following statements relationship is not correct?

Options

A. In an exothermic reaction, the enthalpy of products is less than that of the reactants
B. `Delta_("fusion") H = Delta_("sub")H-Delta_("vap")H`
C. A reaction for which `DeltaH^(Theta) lt 0` and `DeltaS^(Theta) gt 0`
D. `DeltaH` is less that `DeltaU` for the reaction `C(s) +1//2O_(2)(g) rarr CO(g)`

Explanation

To determine which of the given statements is incorrect, we will analyze each statement one by one based on the principles of thermodynamics.

### Step 1: Analyze the First Statement
**Statement:** In an exothermic reaction, the enthalpy of the product is less than that of the reactant.

**Analysis:**
- In an exothermic reaction, heat is released, which means the products have lower energy than the reactants.
- Mathematically, we can express this as:
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