## Related questions with answers

A nonvolatile organic compound $Z$ was used to make up two solutions. Solution $\mathrm{A}$ contains $5.00 \mathrm{~g}$ of $\mathrm{Z}$ dissolved in $100 \mathrm{~g}$ of water, and solution B contains $2.31 \mathrm{~g}$ of $Z$ dissolved in $100 \mathrm{~g}$ of benzene. Solution $\mathrm{A}$ has a vapor pressure of $754.5 \mathrm{mmHg}$ at the normal boiling point of water, and solution B has the same vapor pressure at the normal boiling point of benzene. Calculate the molar mass of $\mathrm{Z}$ in solutions $\mathrm{A}$ and $\mathrm{B}$ and account for the difference.

Solution

VerifiedIn this exercise, the goal is to determine the molar mass of the compound in the two solutions and compare. Since the problem provided us with the vapor pressures of the solution, we need to use the formula for the vapor-pressure lowering, which is given by the equation:

$P_\text{i}=x_\text{i}P^*_\text{i} \tag 1$

where,

$\quad P_\text{i}$ is the vapor pressure of the solution

$\quad x_\text{i}$ is the mole fraction of the solvent

$\quad P^*_\text{i}$ is the vapor pressure of the pure solvent

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