Question

1. $\boldsymbol{2 c_6h_6o + 11 o_2

ightarrow 12 co + 6 h_2o}$
how many moles of oxygen ($o_2$) reacted if 0.6 moles of water ($h_2o$) were produced?

Explanation:

Step1: Use balanced equation mole ratio

Balanced equation: $2\text{C}_6\text{H}_6\text{O} + 11\text{O}_2
ightarrow 12\text{CO} + 6\text{H}_2\text{O}$
Mole ratio of $\text{O}_2:\text{H}_2\text{O} = 11:6$

Step2: Set up proportion for calculation

Let $n(\text{O}_2)$ = moles of oxygen reacted.
$\frac{n(\text{O}_2)}{n(\text{H}_2\text{O})} = \frac{11}{6}$

Step3: Substitute known value and solve

$n(\text{H}_2\text{O}) = 0.6$ mol
$n(\text{O}_2) = \frac{11}{6} \times 0.6$
$n(\text{O}_2) = 1.1$

Answer:

1.1 moles