At a particular temperature,the vapour pressures of two liquids $A$ and $B$ are respectively $120 \, mm$ and $180 \, mm$ of mercury. If $2 \, moles$ of $A$ and $3 \, moles$ of $B$ are mixed to form an ideal solution,the vapour pressure of the solution at the same temperature will be (in $mm$ of mercury):
- A$156$
- B$145$
- C$150$
- D$108$
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Which of the following pairs of liquids shows a negative deviation from Raoult's law?
Easy
View SolutionWhich of the following is/are "not correct" for $CH_3OH + CH_3COOH$ mixture solution?
$(a)$ $\Delta H_{\text{mix}} < 0$
$(b)$ Does not obey Raoult's law
$(c)$ $\Delta H_{\text{mix}} > 0$
$(d)$ An example of ideal solution
$(a)$ $\Delta H_{\text{mix}} < 0$
$(b)$ Does not obey Raoult's law
$(c)$ $\Delta H_{\text{mix}} > 0$
$(d)$ An example of ideal solution
The vapour pressures of chloroform $(CHCl_3)$ and dichloromethane $(CH_2Cl_2)$ at $298 \ K$ are $200 \ mmHg$ and $415 \ mmHg$,respectively. An ideal solution is prepared by mixing $59.75 \ g$ of $CHCl_3$ and $21.25 \ g$ of $CH_2Cl_2$. The mole fractions of chloroform and dichloromethane in the vapour phase,respectively,are:
Assuming ideal behaviour,the enthalpy and volume of mixing of two liquids respectively,are
MediumKVPY 2011
View SolutionWhat are the values of $\Delta H_{mix}$ and $\Delta V_{mix}$ for an ideal solution?
Easy
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