# 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?

Oct 15, 2016

Clearly, $0.74 \cdot m o l$ of tin metal will result in the presence of stoichiometric dihydrogen.

#### Explanation:

So, why clearly?

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

$S n {O}_{2} \left(s\right) + 2 {H}_{2} \left(g\right) \rightarrow S n \left(s\right) + 2 {H}_{2} O \left(l\right)$

This is a so-called $\text{redox reaction}$: 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 $150.71 \cdot g \cdot m o {l}^{-} 1$, normally you would be asked how much metal would be produced. So, how much metal in grams?