Question

Another component of acid rain is nitric acid, which forms when NO2, also a pollutant, reacts with oxygen and water according to the simplified equation 4NO2(g)+O2(g)+2H2O(l) → 4HNO3(aq) The generation of the electricity used in a medium-sized home produces about 14 kg of NO2 per year. Part A Assuming that there is adequate O2 and H2O, what mass of HNO3, in kg, can form from this amount of NO2 pollutant?

Answer 1

19 kg. The balanced equation is 4NO2(g)+O2(g)+2H2O(l) ==> 4HNO3(aq) Determine the molar mass of NO2 and HNO3. Atomic weight nitrogen = 14.0067 Atomic weight hydrogen = 1.00794 Atomic weight oxygen = 15.999 Molar mass NO2 = 14.0067 + 2 * 15.999 = 46.0047 g/mol Molar mass HNO3 = 1.00794 + 14.0067 + 3 * 15.999 = 63.01164 g/mol moles NO2 = 14000 g / 46.0047 = 304.3167329 mol Looking at the balanced equation 4NO2(g)+O2(g)+2H2O(l) ==> 4HNO3(aq) it's obvious that each mole of NO2 will produce one mole of HNO3. So we should have 304.3167329 moles worth. Just multiply by the molar mass. 304.3167329 mol * 63.01164 g/mol = 19175.49642 g = 19.17549642 kg Since our data only has 2 significant figures, round to 2 figures, giving 19 kg.

Answer 2

The mass of HNO3 will be 17.8 kg.

Further Explanation:

More than one element bonded together is known as a compound.Sum of total mass of molecule measure in gram which constitutes the atom of molecule known as molar mass. Gram per mole is an S.I. unit of molar mass.Molarity of a solution define as the number of moles of solute per litre solution.

For the provided reaction:

$4{\text{N}}{{\text{O}}_2}({\text{g}})+{{\text{O}}_2}({\text{g}})+2{\text{N}}{{\text{O}}_2}({\text{l}})\to4{\text{N}}{{\text{O}}_3}({\text{aq}})$

Oxygen and water found in abundance. So, the NO2 is known as a limiting reagent as it is responsible for limiting the product formation. The moles of NO2is calculated with the help of the formula:

$\begin{gathered}{\text{Number of moles=}}\frac{{{\text{given mass}}}}{{{\text{molar mass}}}}\hfill\\\begin{array}{*{20}{l}}{{\text{Given mass }}=14{\text{ kg}}=14000{\text{ grams}}}\\{{\text{Molar mass}}=46{\text{g/mol}}}\end{array}\hfill\\\end{gathered}$

Inserting the values in the formula,

$\begin{aligned}{\text{Moles of N}}{{\text{O}}_2}=\frac{{14000}}{{46}}\\=304.34\end{aligned}$

By the help of Stoichiometry,  

4 moles of NO2 will generate 4 moles of HNO3

This means that 304.34 moles of  will generate,

$\begin{gathered}=\frac{4}{4}\times304.34\hfill\\=304.34\hfill\\\end{gathered}$

In order to calculate the mass of HNO3, first equation can be used and we will get,

$\begin{aligned}{{\text{Molar mass of HN}}{{\text{O}}_3}&={\text{ }}63{\text{ g/mol}}}\\{&=304.34\times63}\\{&=19173.42\text{ g}{\text{ or }}19.17{\text{ Kg}}}\end{aligned}$

Learn more:

1. Learn more about ionic bonding brainly.com/question/1603987

2. Learn more about grams of oxygen brainly.com/question/8175791

3. Learn more about chemical reaction brainly.com/question/8175791

Answer Details:

Grade: High School

Subject: Chemistry

Chapter: Solution

Keywords:

Stoichiometry, number of moles, nitric oxide, given mass, molar mass, equation, moles, oxygen, water,unit, element, compound, atom, molarity, solution.