Question

The enthalpy of vaporization of Bromine is 15.4 kJ/mol. What is the energy change when 80.2 g of Br2 condenses to a liquid at 59.5°C?

Answer 1

The enthalpy of vaporization of Bromine is 15.4 kJ/mol. -7.7 kJ is the energy change when 80.2 g of Br₂ condenses to a liquid at 59.5°C.

What is Enthalpy of Vaporization ?

The amount of enthalpy or energy that must be added to a liquid substance into gas substance is called Enthalpy of Vaporization. It is also known as Latent heat of vaporization.

How to find the energy change from enthalpy of vaporization ?

To calculate the energy use this expression:

$Q = n \Delta H_{\text{vapo.}$

where,

Q = Energy change

n = number of moles

$\Delta H_{\text{Vapo.}}$ = Molar enthalpy of vaporization

Now find the number of moles

Number of moles (n) = $\frac{\text{Given Mass}}{\text{Molar mass}}$

                                   = $\frac{80.2\ g }{159.8\ g/mol}$

                                   = 0.5 mol

Now put the values in above formula we get

$Q = - n \Delta H_{\text{vapo.}$         [Negative sign is used because Br₂ condensed here]

   = - (0.5 mol × 15.4 kJ/mol)

   = - 7.7 kJ

Thus from the above conclusion we can say that The enthalpy of vaporization of Bromine is 15.4 kJ/mol. -7.7 kJ is the energy change when 80.2 g of Br₂ condenses to a liquid at 59.5°C.

Learn more about the Enthalpy of Vaporization here: brainly.com/question/13776849

#SPJ1