Question

The statement, the total pressure of a mixture of ideal gases is the sum of partial pressures, is called as

• A. Boyle's law
• B. Charles' law
• C. Dalton's law
• D. Perfect gas law
• E. Law of equipartition

Hint:

For a mixture of ideal gases, remember: \[ P_{\text{total}}=\sum P_{\text{partial}} \] This is Dalton’s law of partial pressures.

Answer 1

The Correct Option is C

Step 1: Understand the given statement.
The question states that for a mixture of ideal gases, the total pressure is equal to the sum of the partial pressures of the individual gases.
Mathematically, this is written as: \[ P = P_1 + P_2 + P_3 + \cdots \]

Step 2: Recall the name of this law.
This statement is known as Dalton's law of partial pressures.
It applies to a mixture of non-reacting ideal gases.

Step 3: State Dalton's law clearly.
Dalton’s law says that if several gases are enclosed in the same container, then the total pressure exerted by the mixture is equal to the algebraic sum of the pressures that each gas would exert if it alone occupied the entire volume at the same temperature.

Step 4: Eliminate the incorrect options.
Boyle’s law relates pressure and volume at constant temperature.
Charles’ law relates volume and temperature at constant pressure.
Perfect gas law is \[ PV=nRT \] which is the ideal gas equation.
Law of equipartition deals with distribution of energy among degrees of freedom.
So none of these match the given statement except Dalton’s law.

Step 5: Write a simple example.
If two ideal gases have partial pressures \( P_1 \) and \( P_2 \), then the total pressure is: \[ P = P_1 + P_2 \] This direct addition is exactly Dalton’s law.

Step 6: Match with the given options.
Among the given choices, the correct one is: \[ \text{Dalton's law} \]

Step 7: Final conclusion.
Hence, the required law is \[ \boxed{\text{Dalton's law}} \] Therefore, the correct option is \[ \boxed{(3)\ \text{Dalton's law}} \]