The vapor pressure of water is 1.00 atm at 373 k, and the enthalpy of vaporization is 40.68 kj mol! . estimate the vapor pressure at temperature 363 and 383 k respectively. ansl = 0.697 atm, ans2 = 1.41 atm

The vapor pressure at temperature 363 K is 0.6970 atm

The vapor pressure at 383 K is 1.410 atm

Explanation:

To calculate of the reaction, we use clausius claypron equation, which is:

where,

= vapor pressure at temperature

= vapor pressure at temperature

= Enthalpy of vaporization  

R = Gas constant = 8.314 J/mol K

1)

= initial temperature =363 K

= final temperature =373 K

Putting values in above equation, we get:

The vapor pressure at temperature 363 K is 0.6970 atm

2)

= initial temperature =373 K

= final temperature =383 K

Putting values in above equation, we get:

The vapor pressure at 383 K is 1.410 atm

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

it should have an internal chamber and two thermometers sticking out of the top. the internal chamber will also be closed off from the outside.