Question

A Reaction is given: ½Br_2(l) --> Br_(g) $\Delta$H^o = 112kJ/mol

The bond enthalpy of Br-Br is 193 kJ/mol

A. Formulate the vaporization process of 1 mol bromine Br_2(l).

B. Calculate the enthalpy of the vaporization process bromine. Show calculations
C. Calculate the energy invested \ emitted by the evaporation of 3.2 gr of bromine. Show calculations.
(Explain how you determined whether the energy is invested or emitted in this process).

D.A Reaction is given: ½H_2(g) + ½Br_2(l) --> HBr_(g)  $\Delta$H^o = -36.2kJ

The bond enthalpy of H-Br is 366 kJ/mol. Calculate the  bond enthalpy of H-H.

E.A Reaction is given: ½H_2(g) + ½Br2_(l) --> HBr_(l)

Will the energy released in the process be high / low / equal to 36.2 kJ?
F. Determine which of the HBr or HCl compounds have a higher enthalpy of vaporization$\Delta$H^o_b . Explain
In terms of structure and bond.

Thank you!!!

Answer 1

male 349 13 23 k丁 1 6a 0-62 kJ

424 A193 362

2 kJ 2