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

Answer:

The heat is  $H= -8.044KJ$

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

               $No \ mole (n) = \frac{Mass \ of \ sample }{Molar \ mass }$

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

Substituting the value into the above equation

          $n = \frac{22.5}{74.12}$

                           $= 0.30356 \ mol$

      The heat H is mathematically as

                $H =- nH_{vap}$

The negative sign show that the heat is for condensing

            $H = 0.30356 * 26.5 *10^{3} J/mol$

                $H= -8.044KJ$