(B) According to Raoult's Law,the total pressure $P$ of a binary solution is given by $P = P_A^0 X_A + P_B^0 X_B$.Since $X_A + X_B = 1$,we have $X_B =

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(B) According to Raoult's Law,the total pressure $P$ of a binary solution is given by $P = P_A^0 X_A + P_B^0 X_B$.Since $X_A + X_B = 1$,we have $X_B = 1 - X_A$.Substituting this into the equation: $P = P_A^0 X_A + P_B^0 (1 - X_A) = (P_A^0 - P_B^0) X_A + P_B^0$.Comparing this with the given equation $P = 0.172 X_A + 0.215$,we can see that the constant term represents the vapor pressure of pure $B$ $(P_B^0)$.Therefore,$P_B^0 = 0.215 \ atm$.

Class 12 Chemistry Solutions Lowering of vapour pressure

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Two liquids $A$ and $B$ form a solution at $306 \ K$ that follows the equation $P \ (\text{in } atm) = 0.172X_A + 0.215$,where $P$ is the total vapor pressure of the solution and $X_A$ is the mole fraction of $A$. The vapor pressure of pure $B$ is ............ . (in $atm$)

A
$0.172$
B
$0.215$
C
$0.043$
D
$0.387$

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Lowering of vapour pressure

Write the formula which expresses the relationship between the total pressure of a solution $(P_{total})$ and the mole fraction $(x_2)$ of the components,according to Raoult's law.

Easy

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$p_A$ and $p_B$ are the vapour pressures of pure liquid components $A$ and $B$ respectively of an ideal binary solution. If $x_A$ represents the mole fraction of component $A,$ the total pressure of the solution will be

Easy

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The vapour pressure of water at $20^\circ C$ is $17.5 \ mm \ Hg$. If $18 \ g$ of glucose $(C_6H_{12}O_6)$ is added to $178.2 \ g$ of water at $20^\circ C$,what will be the vapour pressure of the resulting solution (in $mm \ Hg$)?

Medium

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The relative lowering of vapor pressure is equal to the mole fraction of the non-volatile solute. This statement was given by whom?

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At $300 \ K$,the vapor pressures of two pure liquids $A$ and $B$ are $150 \ mm \ Hg$ and $100 \ mm \ Hg$,respectively. If the mole fractions of $A$ and $B$ in the solution are equal,then the mole fraction of $B$ in the vapor phase at the same temperature is:

Medium

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Two liquids $A$ and $B$ form a solution at $306 \ K$ that follows the equation $P \ (\text{in } atm) = 0.172X_A + 0.215$,where $P$ is the total vapor pressure of the solution and $X_A$ is the mole fraction of $A$. The vapor pressure of pure $B$ is ............ . (in $atm$)

Similar Questions

Write the formula which expresses the relationship between the total pressure of a solution $(P_{total})$ and the mole fraction $(x_2)$ of the components,according to Raoult's law.

$p_A$ and $p_B$ are the vapour pressures of pure liquid components $A$ and $B$ respectively of an ideal binary solution. If $x_A$ represents the mole fraction of component $A,$ the total pressure of the solution will be

The vapour pressure of water at $20^\circ C$ is $17.5 \ mm \ Hg$. If $18 \ g$ of glucose $(C_6H_{12}O_6)$ is added to $178.2 \ g$ of water at $20^\circ C$,what will be the vapour pressure of the resulting solution (in $mm \ Hg$)?

The relative lowering of vapor pressure is equal to the mole fraction of the non-volatile solute. This statement was given by whom?

At $300 \ K$,the vapor pressures of two pure liquids $A$ and $B$ are $150 \ mm \ Hg$ and $100 \ mm \ Hg$,respectively. If the mole fractions of $A$ and $B$ in the solution are equal,then the mole fraction of $B$ in the vapor phase at the same temperature is:

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