Two compounds form an ideal solution at room temperature. Which of the following are correct for this ideal solution?
$(A)$ $\Delta G_{mix} < 0$
$(B)$ $\Delta S_{mix} > 0$
$(C)$ $\Delta V_{mix} = 0$
$(D)$ $\Delta_{mix} H = 0$

Liquids $A$ and $B$ form an ideal solution. At $30\,^oC$,the total vapour pressure of a solution containing $1\,mol$ of $A$ and $2\,mol$ of $B$ is $250\,mm\,Hg$. The total vapour pressure becomes $300\,mm\,Hg$ when $1$ more $mol$ of $A$ is added to the first solution. The vapour pressures of pure $A$ and $B$ at the same temperature are

Assuming the formation of an ideal solution,determine the boiling point of a mixture containing $1560 \ g$ benzene (molar mass $= 78 \ g/mol$) and $1125 \ g$ chlorobenzene (molar mass $= 112.5 \ g/mol$) against an external pressure of $1000 \ torr$. Use the provided vapor pressure vs. temperature graph to find the answer. (in $^{\circ}C$)

At $T(K)$,the vapour pressures of two liquids,heptane and octane are $106 \ kPa$ and $47 \ kPa$ respectively. If $25 \ g$ of heptane and $57 \ g$ of octane form an ideal solution,at $T(K)$ the vapour pressure of solution in $kPa$ is :

What is meant by positive and negative deviations from Raoult's law and how is the sign of $\Delta_{mix} H$ related to positive and negative deviations from Raoult's law?

Which of the following mixtures is an ideal solution?