Q. 7.63 - An Introduction to General, Organic, and Biological Chemistry

Question

Nitrogen dioxide and water react to produce nitric acid, $HN{O}_3$ and nitrogen oxide.

$3N{O}_2\left(g\right)+H_{2}O\left(l\right)\to 2HN{O}_3\left(aq\right)+NO\left(g\right)$

a. How many grams of $H_{2}O$ are needed to react with $28.0 \mathrm{g}$ of  $N{O}_2$ ?

b. How many grams of $NO$ are produced from $15.8 \mathrm{g}$of  $H_{2}O$ ?

c. How many grams of $HN{O}_3$are produced from$8.25 \mathrm{g}$ of $N{O}_2$ ?

Step-by-Step Solution

Answer

(a) The $3.64 \mathrm{g} {\mathrm{H}}_2\mathrm{O}$are needed to react with $28.0 \mathrm{g}$of $N{O}_2$.

(b) The $25.28 \mathrm{g} \mathrm{NO}$are produced from $15.8 \mathrm{g}$ of ${\mathrm{H}}_2\mathrm{O}$

(c) The $7.5 \mathrm{g} {\mathrm{HNO}}_3$ are produced from $8.25 \mathrm{g}$ of ${\mathrm{NO}}_2$.

Part(a) Step 1: Given information

We have to find out the how many grams of $H_{2}O$ are needed to react with $28.0 \mathrm{g}$of $N{O}_2$.

Part(a) Step 2: Explanation

Now, we find answer,

$[3\times 46 \mathrm{g}] {\mathrm{NO}}_2\to [18 \mathrm{g}] {\mathrm{H}}_2\mathrm{O}$,

$[1 \mathrm{g}] {\mathrm{NO}}_2\to \left(\frac{18 \cancel{\mathrm{g}}}{3\times 46 \cancel{\mathrm{g}}}\right) {\mathrm{H}}_2\mathrm{O}$,

$[28 \mathrm{g}] {\mathrm{NO}}_2\to \left[\frac{18 \cancel{\mathrm{g}}}{3\times 46 \cancel{\mathrm{g}}}\times 28 \mathrm{g}\right] {\mathrm{H}}_2\mathrm{O}$,

$=3.64 \mathrm{g} {\mathrm{H}}_2\mathrm{O}$.

Part(b) Step 2: Given information

We have to find out the how many grams of $NO$are produced from $15.8 \mathrm{g}$of $H_{2}O.$

Part(b) Step 2: Explanation

Now, we calculated to find answer,

$[18 \mathrm{g}] {\mathrm{H}}_2\mathrm{O}\to [30 \mathrm{g}] \mathrm{NO}$,

$[1 \mathrm{g}] {\mathrm{H}}_2\mathrm{O}\to \left[\frac{30 \cancel{\mathrm{g}}}{18 \cancel{\mathrm{g}}}\right] \mathrm{NO}$,

$15.8 \mathrm{g} {\mathrm{H}}_2\mathrm{O}\to \left[\frac{30 \cancel{\mathrm{g}}}{18 \cancel{\mathrm{g}}}\times 15.8 \mathrm{g}\right] \mathrm{NO}$,

$=25.28 \mathrm{g} \mathrm{NO}$.

Part(c) Step 1: Given information

We have to find out the how many grams of $HN{O}_3$are produced from $8.25g of N{O}_2$.

Part(c) Step 2: Explanation

Now, we calculated to find answer,

$[3\times 46 \mathrm{g}] {\mathrm{NO}}_2\to [2\times 63 \mathrm{g}] {\mathrm{HNO}}_3$,

$[1 \mathrm{g}] {\mathrm{NO}}_2\to \left[\frac{2\times 63 \cancel{\mathrm{g}}}{3\times 46 \cancel{\mathrm{g}}}\right] {\mathrm{HNO}}_3$,

$[8.25 \mathrm{g}] {\mathrm{NO}}_2\to \left[\frac{2\times 63}{3\times 46}\times 8.25\mathrm{g}\right] {\mathrm{HNO}}_3$,

$=7.5 \mathrm{g} {\mathrm{HNO}}_3$.