Two liquids A and B from ideal solutions. At 300 K, the vapour pressure of solution containing

step 1 In this problem I can write the value of p total is equal to p a not x a plus p a not xb. So 550

Two liquids A and B from ideal solutions. At 300 K, the...

Two liquids $A$ and $B$ from ideal solutions. At $300 \mathrm{~K}$, the vapour pressure of solution containing 1 mole of $A$ and 3 mole of $B$ is $550 \mathrm{~mm} \mathrm{Hg}$. At the same temperature, if one more mole of $B$ is added to this solution, the vapour pressure of the solution increases by $10 \mathrm{~mm} \mathrm{Hg}$. Determine the vapour pressure of $A$ and $B$ in their pure states (in $\mathrm{mm} \mathrm{Hg}$ ): (a) 400,600 (b) 500,500 (c) 600,400 (d) None of these

Two liquids $A$ and $B$ from ideal solutions. At $300 \mathrm{~K}$, the vapour pressure of solution containing 1 mole of $A$ and 3 mole of $B$ is $550 \mathrm{~mm} \mathrm{Hg}$. At the same temperature, if one more mole of $B$ is added to this solution, the vapour pressure of the solution increases by $10 \mathrm{~mm} \mathrm{Hg}$. Determine the vapour pressure of $A$ and $B$ in their pure states (in $\mathrm{mm} \mathrm{Hg}$ ):
(a) 400,600
(b) 500,500
(c) 600,400
(d) None of these

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Key Concepts

Partial Pressure

Partial pressure refers to the pressure exerted by an individual component in a mixture of gases, assuming it behaves independently. In the context of solutions, each component contributes to the overall vapor pressure in proportion to its mole fraction and its pure state vapor pressure.

Raoult's Law

Raoult's Law is a principle that states the partial vapor pressure of a component in an ideal solution is proportional to the vapor pressure of the pure component and its mole fraction in the solution. This concept is crucial for calculating the total vapor pressure of a solution by summing the contributions from each component.

Ideal Solutions

An ideal solution is one in which the interactions between different molecules are similar to those between like molecules, resulting in behavior that strictly follows Raoult's Law. This simplifies analysis because the properties of the solution can be directly related to the properties of the pure components.

Mole Fraction

Mole fraction is a way of expressing the concentration of a component in a solution, defined as the ratio of the number of moles of that component to the total number of moles in the mixture. It is a fundamental parameter in applying Raoult's Law to determine partial and total vapor pressures in ideal solutions.

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