Total pressure of a gaseous mix is equal to the sum of the Partial Pressures is:

Explanation

To solve the question regarding the total pressure of a gaseous mixture being equal to the sum of the partial pressures, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Concept**: The question is based on Dalton's Law of Partial Pressures. According to this law, in a mixture of non-reacting gases, the total pressure exerted by the mixture is equal to the sum of the partial pressures of the individual gases present in the mixture.

2. **Defining Total Pressure**: Let \( P_T \) be the total pressure of the gaseous mixture. This can be expressed mathematically as:
\[ P_T = P_A + P_B + P_C + \ldots \]
where \( P_A, P_B, P_C, \ldots \) are the partial pressures of the individual gases A, B, C, etc.

3. **Applying Dalton's Law**: According to Dalton's Law:
\[ P_T = \sum P_i \]
where \( P_i \) represents the partial pressures of each gas in the mixture. This means that if we have gases A, B, and C, then:
\[ P_T = P_A + P_B + P_C \]

4. **Understanding Partial Pressure**: The partial pressure of a gas in a mixture is the pressure that gas would exert if it occupied the entire volume alone at the same temperature. It can be calculated using the formula:
\[ P_i = X_i \cdot P_T \]
where \( X_i \) is the mole fraction of gas \( i \).

5. **Conclusion**: Therefore, the total pressure of a gaseous mixture is indeed equal to the sum of the partial pressures of the individual gases, as stated by Dalton's Law.

### Final Statement:
Thus, we conclude that the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual gases, which is a statement of Dalton's Law.

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