Question

How many moles of tin metal will be produced when 0.74 moles of tin IV oxide is heated in the reaction `SnO_2 + 2H_2 -> Sn + 2H_2O`?

Answer 1

Clearly, `0.74*mol` of tin metal will result in the presence of stoichiometric dihydrogen.

Explanation:

So, why clearly?

Well, to begin, you already have the stoichiometric equation:

`SnO_2(s) +2H_2(g) rarr Sn(s) + 2H_2O(l)`

This is a so-called `"redox reaction"`: stannic oxide is reduced to tin metal; and dihydrogen is oxidized to water.

There is 1:1 equivalence of stannic oxide to tin metal. And thus 1:1 molar equivalence. Since stannic oxide has a molar mass of `150.71*g*mol^-1`, normally you would be asked how much metal would be produced. So, how much metal in grams?