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Question
Using Raoult’s law explain how the total vapour pressure over the solution is related to mole fraction of components in the following solutions.
\[\ce{CHCl3(l) and CH2Cl2(l)}\]
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Solution
For a binary solution having both components as volatile liquids (viz, \[\ce{CHCl3 and CH2Cl2}\]), the total pressure will be
`p = p_1 = x_1p_1^0 + x_2p_2^0`
= `x_1p_1^0 + (1 - x_1)p_2^0`
= `(p_1^0 - p_2^0)x_1 + P_2^0`
p = total vapour pressure of the given mixture/binary solution of the given volatile liquids
p1 = partial vapour pressure of component 1 (i.e. \[\ce{CHCl3}\])
p2 = partial vapour pressure pf the component 2 (i.e. \[\ce{CH2Cl2}\])
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