Question

Iodine is prepared both in the laboratory and commercially by adding Cl2(g) to an aqueous solution containing sodium iodide.

2NaI(aq)+Cl2(g)⟶I2(s)+2NaCl(aq)

How many grams of sodium iodide, NaI, must be used to produce 53.4 g of iodine, I2?

Answer 1

$$2NaI_{aq}+Cl_{2}(aq)\rightarrow I_2(s)+2NaCl_(aq)$$

Molar ratio NaI:I$_2$ =2:1

Molar masses= 149.89g and 253.81g respectively

Mass of NaI=$53.4g\times \frac{1mole I_2}{253.81g}\times\frac{2mol NaI}{1mol I_2}\times\frac{149.89g}{1molNaI}$

=63.07g of NaI