(B) $X$$Y$$n_x = 5$$n_y = 10$$P_x^0 = 63 \ torr$$P_y^0 = 78 \ torr$Mole fraction of $X$ $(x_x)$ = $\frac{5}{5+10} = \frac{1}{3}$Mole fraction of $Y$ $

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The solution shows negative deviation.

(B) $X$$Y$$n_x = 5$$n_y = 10$$P_x^0 = 63 \ torr$$P_y^0 = 78 \ torr$Mole fraction of $X$ $(x_x)$ = $\frac{5}{5+10} = \frac{1}{3}$Mole fraction of $Y$ $(x_y)$ = $\frac{10}{5+10} = \frac{2}{3}$According to Raoult's Law,the calculated vapour pressure $(P_{s(calc.)})$ is:$P_{s(calc.)} = P_x^0 x_x + P_y^0 x_y$$P_{s(calc.)} = (63 \times \frac{1}{3}) + (78 \times \frac{2}{3})$$P_{s(calc.)} = 21 + 52 = 73 \ torr$Given observed vapour pressure $(P_{s(obs.)})$ = $70 \ torr$Since $P_{s(obs.)} < P_{s(calc.)}$,the solution shows negative deviation from Raoult's Law.

Class 12 Chemistry Solutions Ideal and Non-ideal solution

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$5$ moles of liquid $X$ and $10$ moles of liquid $Y$ make a solution having a vapour pressure of $70 \ torr$. The vapour pressures of pure $X$ and $Y$ are $63 \ torr$ and $78 \ torr$ respectively. Which of the following is true regarding the described solution?

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A
The solution shows positive deviation.
B
The solution shows negative deviation.
C
The solution is ideal.
D
The solution has volume greater than the sum of individual volumes.

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If vapour pressures of pure liquids $A$ and $B$ are $300$ and $800 \, torr$ respectively at $25 \, ^{\circ}C$. When these two liquids are mixed at this temperature to form a solution in which mole percentage of $B$ is $92$,then the total vapour pressure is observed to be $0.95 \, atm$. Which of the following is true for this solution?

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On mixing $10 \ mL$ $CCl_4$ and $10 \ mL$ benzene,the total volume of solution is

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In a binary ideal solution of liquids $A$ and $B$ at a constant temperature,the mole fraction of $B$ in the liquid phase is $0.4$ and in the vapor phase is $0.25$. If $P_B^o = 40 \ mm \ Hg$,then the vapor pressure of pure liquid $A$ at that temperature is .......... $mm \ Hg$.

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Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.

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Benzene and toluene form nearly ideal solutions. At $20\,^{\circ}C$,the vapour pressure of benzene is $75\,torr$ and that of toluene is $22\,torr$. The partial vapour pressure of benzene at $20\,^{\circ}C$ for a solution containing $78\,g$ of benzene and $46\,g$ of toluene in $torr$ is

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$5$ moles of liquid $X$ and $10$ moles of liquid $Y$ make a solution having a vapour pressure of $70 \ torr$. The vapour pressures of pure $X$ and $Y$ are $63 \ torr$ and $78 \ torr$ respectively. Which of the following is true regarding the described solution?

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On mixing $10 \ mL$ $CCl_4$ and $10 \ mL$ benzene,the total volume of solution is

In a binary ideal solution of liquids $A$ and $B$ at a constant temperature,the mole fraction of $B$ in the liquid phase is $0.4$ and in the vapor phase is $0.25$. If $P_B^o = 40 \ mm \ Hg$,then the vapor pressure of pure liquid $A$ at that temperature is .......... $mm \ Hg$.

Which of the following are correct for an ideal solution?$(a) \Delta V_{\text{mix}} = 0$$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$$(c) \Delta H_{\text{mix}} = 0$$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.

Benzene and toluene form nearly ideal solutions. At $20\,^{\circ}C$,the vapour pressure of benzene is $75\,torr$ and that of toluene is $22\,torr$. The partial vapour pressure of benzene at $20\,^{\circ}C$ for a solution containing $78\,g$ of benzene and $46\,g$ of toluene in $torr$ is

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Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.