Chemistry: Molecular Iodine and Atomic Iodine

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SUMMARY

The discussion centers on the relationship between moles of molecular iodine (I2) and moles of atomic iodine (I) in the context of the balanced chemical equation IO3-(aq) + 5I-(aq) + 6H+(aq) = 3I2(aq) + 3H2O(l). It is established that one mole of molecular iodine produces two moles of atomic iodine, as indicated by the dissociation reaction I2 → 2I. Therefore, the moles of atomic iodine are twice the moles of molecular iodine in this reaction.

PREREQUISITES
  • Understanding of chemical equations and balancing reactions
  • Knowledge of mole concept in chemistry
  • Familiarity with iodine species: molecular iodine (I2) and atomic iodine (I)
  • Basic grasp of aqueous solutions and their components
NEXT STEPS
  • Study the mole concept and its applications in chemical reactions
  • Learn about balancing chemical equations, focusing on redox reactions
  • Explore the properties and reactions of iodine in different states
  • Investigate the implications of stoichiometry in chemical equations
USEFUL FOR

Chemistry students, educators, and professionals involved in chemical research or education, particularly those focusing on reaction stoichiometry and iodine chemistry.

Ly444999
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So I just had a question about calculating moles atomic iodine when you have the moles of molecular iodine. In the chemical equation IO3-(aq) + I-(aq) + H+(aq) = I2(aq) + H2O(l)

Would the moles of atomic iodine be equal to the moles of the molecular iodine? or would the moles of atomic iodine be twice as much as molecular iodine?

Edit: Just realized the equation is unbalanced:
IO3-(aq) + 5I-(aq) + 6H+(aq) = 3I2(aq) + 3H2O(l)
 
Last edited:
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What about

I2 → 2I

Does it answer your question?
 
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