This question is asking for the number of atoms of silver metal that are required to react completely with 531.8 g of iodine to produce silver iodide. At the end, the result turns out to be 2.524x10²⁴ atoms:
In chemistry, stoichiometry is a tool for us to perform mole-mass-particles relationships in chemical reactions. Thus, these problems require a balanced chemical equation, molar masses and the Avogadro's number to proceed.
In such a way. we start by writing the balanced equation for this problem:
[tex]2Ag+I_2\rightarrow 2AgI[/tex]
Hence, we can calculate the atoms of silver with the following stoichiometric setup:
[tex]531.8gI_2*\frac{1molI_2}{253.81gI_2}*\frac{2molAg}{1molI_2} *\frac{6.022x10^{23}atomsAg}{1molAg}[/tex]
Where 253.81 is the molar mass of diatomic iodine, 2:1 the mole ratio of silver to iodine and 6.022x10²³ the Avogadro's number. Thus, after solving, we obtain:
[tex]2.524x10^{24}atomsAg[/tex]
Learn more about stoichiometry: brainly.com/question/9743981
