Given below are the temperatures at which two different liquid compounds with the same empirical formula have a vapor pressure of 400 torr. Which of the following statements is false?
A) Increasing the temperature will increase the vapor pressure of both liquids.
B) Intermolecular attractive forces are stronger in (liquid) ethanol than in (liquid) dimethyl ether.
C) The normal boiling point of dimethyl ether will be higher than the normal boiling point of ethanol.
D) The reason why the temperature at which the vapor pressure is 400 torr is higher for ethanol (than for dimethyl ether) is that there is strong hydrogen bonding in ethanol.
E) None of these statements is false.

Question

Given below are the temperatures at which two different liquid compounds with the same empirical formula have a vapor pressure of 400 torr.  Which of the following statements is false?
A) Increasing the temperature will increase the vapor pressure of both liquids. 
B) Intermolecular attractive forces are stronger in (liquid) ethanol than in (liquid) dimethyl ether. 
C) The normal boiling point of dimethyl ether will be higher than the normal boiling point of ethanol. 
D) The reason why the temperature at which the vapor pressure is 400 torr is higher for ethanol (than for dimethyl ether) is that there is strong hydrogen bonding in ethanol. 
E) None of these statements is false.

Quizplus · Accepted Answer

According to the Clausius-Clapeyron equation, the boiling point of a liquid is directly proportional to its vapor pressure. Therefore, the liquid with a higher boiling point will have a lower vapor pressure at a given temperature. Since the temperature at which both liquids have a vapor pressure of 400 torr is higher for dimethyl ether, it suggests that its boiling point is higher than that of ethanol. Therefore, statement C is false. Statements A, B, D, and E are all true.

Given Below Are the Temperatures at Which Two Different Liquid