The vapor pressure of the liquid so2 is measure at different temperatures. the following vapor pressure data are obtained. temp (k) pressure mmhg241.3 271.2259.3 641.8calculate the enthalpy of vaporization(delta h vap) in kj/mol for this liquid.

24.895 kJ/mol

Explanation:

The expression for Clausius-Clapeyron Equation is shown below as:

Where,  

P is the vapor pressure

ΔHvap  is the Enthalpy of Vaporization

R is the gas constant (8.314 J /mol K)

c is the constant.

For two situations and phases, the equation becomes:

Given:

= 271.2 mmHg

= 641.8 mmHg

= 241.3 K  

= 259.3 K

So,  

ΔHvap = 24895.015 J/mol = 24.895 kJ/mol ( 1 J = 0.001 kJ )

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol