Question

missed this? watch kcv: reaction stoichiometry, read section 8.3. you can click on the review link to access the section in your e text. for the reaction shown, calculate how many moles of no₂ form when each amount of reactant completely reacts. 2 n₂o₅ (g) → 4 no₂ (g) + o₂ (g) part d 1.005 × 10⁻³ mol n₂o₅ express your answer using four significant figures.

Explanation:

Step1: Identify mole ratio

From reaction $2\text{N}_2\text{O}_5(g)
ightarrow 4\text{NO}_2(g) + \text{O}_2(g)$, ratio of $\text{NO}_2$ to $\text{N}_2\text{O}_5$ is $4:2 = 2:1$.

Step2: Calculate moles of $\text{NO}_2$

Moles of $\text{NO}_2 = 1.005 \times 10^{-3}\ \text{mol}\ \text{N}_2\text{O}_5 \times 2 = 2.010 \times 10^{-3}\ \text{mol}$

Step3: Round to 4 significant figures

$2.010 \times 10^{-3}$ has 4 significant figures.

Answer:

$2.010 \times 10^{-3}$ mol