The ideal pressure exerted by a number of non-reacting gases is equal to the sum of the partial pressures of the gases under the same conditions. This statement is according to :

Options

A. Boyle's Law
B. Charle' Law
C. Avogardro's Law
D. Dalton's Law of partial pressures.

Explanation

To solve the question regarding the statement about the ideal pressure exerted by a number of non-reacting gases and its relation to Dalton's law of partial pressures, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Concept of Partial Pressure**:
- Partial pressure is the pressure that a single gas in a mixture would exert if it occupied the entire volume alone at the same temperature.

2. **Dalton's Law of Partial Pressures**:
- Dalton's law states that in a mixture of non-reacting gases, the total pressure exerted by the gas mixture is equal to the sum of the partial pressures of each individual gas.
- Mathematically, this can be expressed as:
\[ P_{total} = P_1 + P_2 + P_3 + ... + P_n \]
where \( P_{total} \) is the total pressure and \( P_1, P_2, P_3, ..., P_n \) are the partial pressures of the individual gases.

3. **Application of Dalton's Law**:
- If we have a container with gases A, B, and C, the total pressure in the container can be calculated by adding the partial pressures of gases A, B, and C.
- This principle applies under the condition that the gases do not react with each other.

4. **Conclusion**:
- Therefore, the statement in the question is indeed according to Dalton's law of partial pressures.

### Final Answer:
The statement is according to **Dalton's Law of Partial Pressures**.

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