Question

Which of the following statements concerning the reaction shown below are true?

AgBr (s) + ½ Cl2 (g) → AgCl (s) + ½ Br2 (l) ∆H = -27.6 kJ

I. heat is absorbed
II. heat is released
III. rxn is exothermic
IV. rxn is endothermic
V. products have higher enthalpy content than reactants
VI. reactants have higher enthalpy content than products

I, III, and V

II, III, and V

II, III, and VI

I and III

Answer 1

Hi what do u think the answer is ?

Answer 2

@Rushwr i have no idea but i am just guessing that it is II, III, and VI?

Answer 3

Here they have given the delta H value for the reaction right? It has mention that delta H is negative. \[\Delta H= \Delta H _{products} - \Delta H _{reactants}\] right?
For delta H to be negative it's pretty clear that delta H products should have a lower value than delta H reactants. Remember when the delta H is negative it is an exothermic process hence this reaction is exothermic. Also in an exothermic reaction the heat is released to the environment. So the answer you gave is correct !

Answer 4

okay cool that is what i thought thank you @Rushwr

Answer 5

Awesome then :)