Question

When 2.85 moles of chlorine reacts with excess tin how many moles of tin(iv) chloride are formed ?

Answer 1

Would it not be a `1.425*mol` quantity?

Explanation:

We assume QUANTITATIVE oxidation of tin metal by chlorine gas (which is of course dichlorine)...i.e.

`Sn(s) + 2Cl_2(g) rarr SnCl_4(l)`

And clearly, if a `2.85*mol` quantity of the chlorine oxidant reacts...an equivalent quantity of `"stannic chloride"` results. You should add the masses of the reactants and products to this answer.