# How many grams of H_2O will be produced if 750 grams of Fe are produced in the equation Fe_3O_4 + H_2 -> Fe + H_2O?

Sep 10, 2017

Approx.....$300 \cdot g$ water are evolved......

#### Explanation:

We need (i) a stoichiometric equation......

$F {e}_{3} {O}_{4} + 4 {H}_{2} \rightarrow 3 F e + 4 {H}_{2} O$

And thus for each mole of iron produced, $\frac{4}{3}$ mol of water are produced consequently......

And (ii) we work out the equivalent quantity of metal.....

$\text{Moles of iron} \equiv \frac{750 \cdot g}{55.8 \cdot g \cdot m o {l}^{-} 1} = 13.44 \cdot m o l$

And so we take the product.....

$13.44 \cdot m o l \times \frac{4}{3} \times 18.011 \cdot g \cdot m o {l}^{-} 1 = 323 \cdot g$ with respect to water.....