In an exothermic reaction heat is evolved and system loses heat to the surrounding. For such system

Options

A. `q_(p)` will be negative
B. `Delta_(r) H` will be negative
C. `q_(p)` will be positive
D. `Delta_(r) H` will be positive

Explanation

To solve the question regarding the characteristics of an exothermic reaction, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Exothermic Reactions**:
- An exothermic reaction is defined as a chemical reaction that releases heat to the surroundings. This means that the system (the reactants) loses energy in the form of heat.

2. **Identifying Heat Transfer (Q)**:
- In thermodynamics, the symbol \( Q \) represents the heat exchanged between the system and its surroundings. Since the system is losing heat, we denote this as:
\[ Q < 0 \]
- This indicates that the heat \( Q \) is negative because the system is releasing heat.

3. **Understanding Enthalpy Change (ΔH)**:
- The change in enthalpy (\( \Delta H \)) for a reaction is a measure of the total heat content of the system. For exothermic reactions, the enthalpy change is also negative, which can be expressed as:
\[ \Delta H < 0 \]
- This means that the products of the reaction have lower energy than the reactants, indicating that energy has been released.

4. **Conclusion**:
- From the above analysis, we conclude that for an exothermic reaction:
- \( Q \) is negative (the system loses heat).
- \( \Delta H \) is negative (the enthalpy change is negative).

### Final Answer:
For an exothermic reaction, both \( Q \) and \( \Delta H \) are negative.