Dalton's Law of Partial Pressures is a principle in chemistry that describes the behavior of gases in a mixture. According to this law, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas in the mixture.
Let's analyze the given options:
A. [tex]\( PV = k \)[/tex]
This is an expression of Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature.
B. [tex]\( V = kn \)[/tex]
This could be a form of Avogadro's Law, which states that the volume of a gas is directly proportional to the number of moles of gas at constant temperature and pressure.
C. [tex]\( P_{\text{total}} = P_1 + P_2 + P_3 + \ldots \)[/tex]
This is Dalton's Law of Partial Pressures. It expresses that the total pressure of a mixture of gases is the sum of the partial pressures of the individual gases.
D. [tex]\( \frac{V}{T} = k \)[/tex]
This is an expression of Charles's Law, which states that the volume of a gas is directly proportional to its temperature at constant pressure.
Given these explanations, the correct expression that represents Dalton's Law is:
C. [tex]\( P_{\text{total}} = P_1 + P_2 + P_3 + \ldots \)[/tex]
