Question

The mass of $FeO$ produced from $2$ g $VO$ and $5.75$ g of ${Fe}_2{O}_3$ is (as nearest integer) :
$VO+{Fe}_2{O}_3\to FeO+V_2{O}_5$

Answer 1

The balanced equation is as follows:
$2VO+3{Fe}_2{O}_3\to 6FeO+V_2{O}_5$
Mole before reaction:

$\frac{2}{67}\frac{5.75}{160}$
$=0.0298=0.0359$
Mole after reaction:
$\left[0.0298-\frac{0.0359\times 2}{3}\right]0(0.0359\times 2)(0.0359\times 1)$

Mole ratio of the reaction is given below:
$VO:{Fe}_2{O}_3:FeO:V_2{O}_5::2:3:6:1$

Moles of $FeO$ formed $=0.0359\times 2$
Mass of $FeO$ formed $=0.0359\times 2\times 72=5.18$ g
So, the nearest integer is $5$.