Question

The following information is given for ether, C2H5OC2H5, at 1atm: boiling point = 34.6 °C Hvap(34.6 °C) = 26.5 kJ/mol specific heat liquid = 2.32 J/g°C /At a pressure of 1 atm, what is H in kJ for the process of condensing a 22.5 g sample of gaseous ether at its normal boiling point of 34.6 °C.

Answer 1

The heat is
`H= -8.044KJ`

Step-by-step explanation:

From the question we are told that

The pressure is
`P = 1 \ atm`

The boiling point is
`B_P = 34^oC`

The heat of vaporization at 34°C is =
`26.5 kJ/mol`

The specific heat of the liquid is
`c_p = 2.32 J/g^oC`

The mass is
`m = 22.5g`

The no of moles of the sample of
`C_2 H_5OC_2H_5` is given as

`No \ mole (n) = (Mass \ of \ sample )/(Molar \ mass )`

The Molar mass for
`C_2 H_5OC_2H_5` is a value =
`= 74.12 g/mol`

Substituting the value into the above equation

`n = (22.5)/(74.12)`

`= 0.30356 \ mol`

The heat H is mathematically as

`H =- nH_(vap)`

The negative sign show that the heat is for condensing

`H = 0.30356 * 26.5 *10^(3) J/mol`

`H= -8.044KJ`