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anonymous

  • one year ago

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

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  1. Rushwr
    • one year ago
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    Hi what do u think the answer is ?

  2. anonymous
    • one year ago
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    @Rushwr i have no idea but i am just guessing that it is II, III, and VI?

  3. Rushwr
    • one year ago
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    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 !

  4. anonymous
    • one year ago
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    okay cool that is what i thought thank you @Rushwr

  5. Rushwr
    • one year ago
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    Awesome then :)

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