Question

use the following information to answer the next question. given the following balanced reaction: 3no₂(g)+ h₂o(l)→2hno₃(aq)+ no(g) numeric response 2. how many grams of nitrogen dioxide are required in this reaction to produce 2.02 g hno₃. (record your answer in the numerical - response section below.) your answer:

Explanation:

Step1: Calculate molar mass of $HNO_3$

The molar mass of $HNO_3$: $M_{HNO_3}=1 + 14+3\times16=63\ g/mol$.

Step2: Calculate moles of $HNO_3$

The number of moles of $HNO_3$, $n_{HNO_3}=\frac{m_{HNO_3}}{M_{HNO_3}}=\frac{2.02\ g}{63\ g/mol}\approx0.0321\ mol$.

Step3: Determine mole - ratio from the balanced equation

From the balanced equation $3NO_2(g)+H_2O(l)
ightarrow2HNO_3(aq) + NO(g)$, the mole - ratio of $NO_2$ to $HNO_3$ is $\frac{n_{NO_2}}{n_{HNO_3}}=\frac{3}{2}$.

Step4: Calculate moles of $NO_2$

$n_{NO_2}=\frac{3}{2}n_{HNO_3}=\frac{3}{2}\times0.0321\ mol = 0.04815\ mol$.

Step5: Calculate mass of $NO_2$

The molar mass of $NO_2$ is $M_{NO_2}=14 + 2\times16=46\ g/mol$. The mass of $NO_2$, $m_{NO_2}=n_{NO_2}\times M_{NO_2}=0.04815\ mol\times46\ g/mol\approx2.22\ g$.

Answer:

$2.22$