The vapor pressure of ethanol is 30°c at 98.5 mmhg and the heat of vaporization is 39.3 kj/mol. determine the normal boiling point of ethanol from this data.

Answer : The normal boiling point of ethanol will be, or

Explanation :

The Clausius- Clapeyron equation is :

where,

= vapor pressure of ethanol at = 98.5 mmHg

= vapor pressure of ethanol at normal boiling point = 1 atm = 760 mmHg

= temperature of ethanol =

= normal boiling point of ethanol = ?

= heat of vaporization = 39.3 kJ/mole = 39300 J/mole

R = universal constant = 8.314 J/K.mole

Now put all the given values in the above formula, we get:

Hence, the normal boiling point of ethanol will be, or

answer

the ions in solute supperate from eachouthere

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.