Iodine is prepared both in the laboratory and commercially by adding cl2(g)cl2(g) to an aqueous solution containing sodium iodide. 2nai(aq)+cl2(g)⟶i2(s)+2nacl(aq) 2nai(aq)+cl2(g)⟶i2(s)+2nacl(aq) how many grams of sodium iodide, nai, nai, must be used to produce 89.1 g89.1 g of iodine, i2? i2? mass: g nai

Answer : The mass of sodium iodide used to produced must be, 105.22 grams.

Explanation : Given,

Mass of = 89.1 g

Molar mass of = 253.8 g/mole

Molar mass of = 149.89 g/mole

First we have to calculate the moles of .

Now we have to calculate the moles of .

The balanced chemical reaction is,

From the balanced chemical reaction, we conclude that

As, 1 mole of obtained from 2 moles of

So, 0.351 moles of obtained from moles of

Now we have to calculate the mass of .

Therefore, the mass of sodium iodide used to produced must be, 105.22 grams.

where's the diagram?