In a gaseous reaction, an increase in the pressure of the reactant gases increases the rate of reaction.T or F

Answer

To determine whether the statement "In a gaseous reaction, an increase in the pressure of the reactant gases increases the rate of reaction" is true or false, we can analyze the relationship between pressure and reaction rate in gaseous reactions.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
Consider a generic gaseous reaction where reactant A converts to product B. We can express this reaction as:
\[ A(g) \rightarrow B(g) \]

2. **Rate of Reaction**:
The rate of a reaction can be expressed in terms of the change in concentration (or pressure in the case of gases) of the reactants over time. For a gaseous reactant A, the rate can be defined as:
\[ \text{Rate} = -\frac{d[P_A]}{dt} \]
where \( P_A \) is the pressure of gas A.

3. **Rate Law Expression**:
The rate of reaction can also be expressed using a rate law, which is dependent on the concentration (or pressure) of the reactants. For a reaction of order \( n \), the rate can be expressed as:
\[ \text{Rate} = k \cdot P_A^n \]
where \( k \) is the rate constant and \( n \) is the order of the reaction.

4. **Effect of Pressure on Rate**:
If we increase the pressure of the reactant gas A, this effectively increases its concentration. According to the rate law, if \( P_A \) increases, then \( P_A^n \) will also increase, leading to an increase in the rate of reaction.

5. **Conclusion**:
Since increasing the pressure of the reactant gases leads to an increase in the rate of reaction, we conclude that the statement is true.

### Final Answer:
**True**