Question

How do I calculate the mass of zinc and iodine that are consumed to produce zinc iodide.

Answer 1

Hint :To answer this question, we first need to understand what are elements. An element is a pure substance made up entirely of atoms with the same number of protons in their atomic nuclei, as defined by chemistry. Chemical elements, unlike chemical compounds, cannot be broken down chemically into simpler molecules.

Complete Step By Step Answer:
The mass of a substance consumed in a chemical reaction refers to one or more reactants. Because the reactants in your question are zinc and iodine, you must calculate the amount of zinc and iodine used to make zinc iodide. The balanced chemical equation for this zinc-iodine synthesis process is:
\[Zn{\text{ }} + {\text{ }}{I_2} \to {\text{ }}Zn{I_2}\]
To figure out how much zinc was consumed (reacted), we need to know how much iodine was consumed (reacted), or how much zinc iodide was created.
Let us take an example –
\[\
  How{\text{ }}many{\text{ }}grams{\text{ }}of{\text{ }}Zn{\text{ }}must{\text{ }}be{\text{ }}consumed{\text{ }}to{\text{ }}react{\text{ }}with{\text{ }}12.52g{\text{ }}{I_2}\;to{\text{ }}produce{\text{ }}ZnC{l_2}? \\
  1){\kern 1pt} {\kern 1pt} 2Determine{\text{ }}moles{\text{ }}{I_2}{\text{ }}by{\text{ }}dividing{\text{ }}the{\text{ }}given{\text{ }}mass{\text{ }}by{\text{ }}its{\text{ }}molar{\text{ }}mass. \\
  2){\kern 1pt} {\kern 1pt} Calculate{\text{ }}moles{\text{ }}Zn{\text{ }}by{\text{ }}multiplying{\text{ }}moles{\text{ }}{I_2}\;by{\text{ }}the{\text{ }}mole{\text{ }}ratio{\text{ }}between{\text{ }}{I_2}\;and{\text{ }}Zn{\text{ }}in{\text{ }}the{\text{ }}balanced{\text{ }}equation, \\
  {\text{ }}with{\text{ }}Zn{\text{ }}in{\text{ }}the{\text{ }}numerator. \\
  Determine{\text{ }}the{\text{ }}mass{\text{ }}of{\text{ }}the{\text{ }}Zn{\text{ }}required{\text{ }}to{\text{ }}react{\text{ }}with{\text{ }}12.5{\text{ }}g{\text{ }}{I_2}{\text{ }}by{\text{ }}multiplying{\text{ }}the{\text{ }}moles{\text{ }}Zn{\text{ }}by{\text{ }}it{\text{ }}molar{\text{ }}mass. \\
  \begin{array}{*{20}{l}}
  \
  12.5g{\text{ }}{I_2}{\text{ }} \times {\text{ }}1mol{\text{ }}{I_2} \\
  253.808g{\text{ }}{I_2}{\text{ }} \times 1mol{\text{ }}Zn \\
  1 mol{\text{ }}{I_2}{\text{ }} \times {\text{ }}65.38g{\text{ }}Zn/1mol{\text{ }}Zn \\
   = 3.22{\text{ }}g{\text{ }}Zn \\
\ \\
  {3.22g{\text{ }}Zn{\text{ }}are{\text{ }}consumed{\text{ }}when{\text{ }}reacted{\text{ }}with{\text{ }}12.5g{\text{ }}{I_2}}
\end{array} \\
\ \]
So, we conclude that, to figure out how much zinc was consumed (reacted), you must first figure out how much iodine was consumed (reacted), or how much zinc iodide was produced.

Note :
A chemical compound is a substance made up of numerous identical molecules bound together by chemical bonds and made up of atoms from different elements. As a result, a molecule made up of only one element's atoms is not a compound.