At 35^{circ} C,the vapour pressure of CS_{2} | vedclass

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(C) The observed total vapour pressure $(600 \; mm \; Hg)$ is greater than the vapour pressure of either pure component ($512 \; mm \; Hg$ and $344 \;

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a mixture of $100 \; mL \; CS_{2}$ and $100 \; mL$ acetone has a volume $< 200 \; mL$

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(C) The observed total vapour pressure $(600 \; mm \; Hg)$ is greater than the vapour pressure of either pure component ($512 \; mm \; Hg$ and $344 \; mm \; Hg$). This indicates that the solution exhibits a positive deviation from Raoult's law. For solutions showing positive deviation: $1$. $\Delta_{sol} H > 0$ (Endothermic process,heat is absorbed). $2$. $\Delta_{sol} V > 0$ (Volume increases,so the final volume is $> 200 \; mL$). $3$. The solute-solvent interactions are weaker than the solute-solute and solvent-solvent interactions. $4$. Raoult's law is not obeyed. Therefore,the statement that the volume is $< 200 \; mL$ is false.

At $35^{\circ} C$,the vapour pressure of $CS_{2}$ is $512 \; mm \; Hg$ and that of acetone is $344 \; mm \; Hg$. $A$ solution of $CS_{2}$ in acetone has a total vapour pressure of $600 \; mm \; Hg$. The false statement amongst the following is

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