State Dalton's law-

Options

A. the total pressure of gas is directly proportional to mole fraction of gas
B. the total pressure of a mixture of gases is equal to sum of temperature of individual molecule
C. the total pressure of mixture of gases is equal to the sum of partial pressure of individual component gases
D. none

Answer

**Step-by-Step Text Solution:**

1. **Understanding Dalton's Law**: Dalton's Law of Partial Pressures 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 in the mixture.

2. **Defining Partial Pressure**: The partial pressure of a gas is the pressure that gas would exert if it occupied the entire volume of the mixture alone at the same temperature.

3. **Mathematical Expression**: If we have two gases, Gas A and Gas B, with their respective number of moles denoted as \( n_A \) and \( n_B \), and the total pressure of the gas mixture is \( P_t \), then:
- The partial pressure of Gas A, denoted as \( P_A \), can be expressed as:
\[ P_A = \frac{n_A}{n_A + n_B} \times P_t \]
- Similarly, the partial pressure of Gas B, denoted as \( P_B \), can be expressed as:
\[ P_B = \frac{n_B}{n_A + n_B} \times P_t \]

4. **Total Pressure**: The total pressure of the gas mixture can be calculated as:
\[ P_t = P_A + P_B \]

5. **Conclusion**: Therefore, Dalton's Law can be summarized as:
\[ P_t = P_A + P_B \]
This means that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas in the mixture.

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