Question

The total pressure exerted by a number of non-reacting gases in a mixture is equal to the sum of partial pressures of the gases in the mixture. This is known as
1. Boyle's law
2. Dalton's law
3. Charles' law
4. Graham's law 

Answer 1

Correct Answer - Option 2 : Dalton's law

The correct answer is Dalton's law.

CONCEPT:

• Boyle's law states that at a constant temperature, the volume of a given mass of gas is inversely proportional to its pressure.
• P1V1 = P2V2
• Graham’s law of diffusion states that at a constant temperature and pressure, the rate of diffusion of a gas is inversely proportional to the square root of its density.
• \(\frac{r_{A}}{r_{B}}=\sqrt{\frac{d_{A}}{d_{B}}}\) or \(\frac{r_{A}}{r_{B}}=\sqrt{\frac{M_{B}}{M_{A}}}\)
•  Where rA and rB are rates of diffusions of A and B, dA and dB are densities and MA and MB are molecular masses of A and B respectively​
• Charles law: This law states that at constant pressure, the volume of a given mass of a gas is directly proportional to its absolute temperature.
• \(\frac{V1}{T1}=\frac{V2}{T2} \)

EXPLANATION:

• Dalton's law of partial pressures states that The total pressure exerted by a number of non-reacting gases in a mixture is equal to the sum of partial pressures of the gases in the mixture. 
• In a mixture, the pressure exerted by individual gas is called partial pressure.
• p_total = p₁+p₂+p₃+..... (at constant T and V), where p_total is the total pressure exerted by the mixture of gases and p₁, p₂, p₃ are the partial pressures of  gases.