Given below are the temperatures at which two different liquid compounds with the same empirical formula have a vapor pressure of 400 torr. Compound T (°C) Dimethyl ether,CH₃-O-CH₃ -37.8 Ethanol,CH₃CH₂OH 63.5 Which of the following statements (a-d)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 that 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 is false.

Question

Quizplus · Accepted Answer

The normal boiling point of a liquid is the temperature at which its vapor pressure equals the atmospheric pressure. Since ethanol has a higher temperature for the same vapor pressure (400 torr) compared to dimethyl ether, it indicates that ethanol has stronger intermolecular forces (due to hydrogen bonding) and thus a higher normal boiling point. Therefore, statement C is false because it incorrectly claims the opposite.

Given Below Are the Temperatures at Which Two Different Liquid