For a chemical reaction, `Delta C_(p)` is negative `(Delta C_(p) lt 0)`.
The heat required to increase temperature of reactants of this reaction by a certain amount `=q_(1)` and heat required to increase temperature of products of the same reaction by same amount `=q_(2)`, Relate `q_(1)` and `q_(2)`

Answer

To relate \( q_1 \) and \( q_2 \) based on the given information, we can follow these steps:

### Step 1: Understand the Definitions
- **Heat Capacity (\( C_p \))**: It is defined as the amount of heat required to raise the temperature of a substance by 1 degree Celsius (or 1 Kelvin).
- **Change in Heat Capacity (\( \Delta C_p \))**: This is defined as the difference in heat capacities between products and reactants in a chemical reaction.

### Step 2: Write the Expression for \( \Delta C_p \)
- According to the problem, we know that:
\[ \Delta C_p = C_{p, \text{products}} - C_{p, \text{reactants}} \]
- We can express this in terms of \( q_1 \) and \( q_2 \):
\[ \Delta C_p = q_2 - q_1 \]

### Step 3: Analyze the Given Condition
- We are given that \( \Delta C_p < 0 \). This means:
\[ q_2 - q_1 < 0 \]
- Rearranging this inequality gives us:
\[ q_2 < q_1 \]

### Step 4: Conclusion
- From the above steps, we can conclude that:
\[ q_1 > q_2 \]
- This means that the heat required to increase the temperature of the reactants (\( q_1 \)) is greater than the heat required to increase the temperature of the products (\( q_2 \)).

### Final Relation
Thus, the relationship between \( q_1 \) and \( q_2 \) is:
\[ q_1 > q_2 \]