Chemistry, 15.10.2019 02:30, lexhorton2002

What is the percent composition by mass of nitrogen in (nh4)2co3 (gram-formula mass = 96.0 g/mol)?

(1) 14.6%
(2) 29.2%
(3) 58.4%
(4) 87.5%

Answers: 1

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Answers

The percentage composition by mass of nitrogen in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is $\boxed{\left( 2 \right){\text{ 29}}{\text{.2 \% }}}$ .

Further explanation:

The most commonly applied concentration terms are as follows:

1. Molality

2. Mole fraction

3. Molarity

4. Parts per million

5. Mass percent

6. Volume percent

7. Percentage composition

The given compound is ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ . It contains two atoms of nitrogen, eight atoms of hydrogen, one atom of carbon and three atoms of oxygen.

The mass of nitrogen in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ can be calculated as follows:

${\text{Mass of N}} =\left( {{\text{Number of nitrogen atoms}}} \right)\left( {{\text{Molar mass of nitrogen}}} \right)$ …… (1)

The number of N atoms in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is 2.

The molar mass of nitrogen is 14.01 g/mol.

Substitute these values in equation (1).

$\begin{aligned}{\text{Mass of nitrogen}} &= \left( {\text{2}} \right)\left( {{\text{14}}{\text{.01 g/mol}}} \right)\\&= 28.02{\text{ g/mol}}\\\end{aligned}$

The formula to calculate the percentage composition of N in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is as follows:

${\text{\% composition of N}} = \left( {\dfrac{{{\text{Mass of N}}}}{{{\text{Mass of }}{{\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)}_{\text{2}}}{\text{C}{{\text{O}}_{\text{3}}}}}} \right){\text{100 \% }}$ …… (2)

The mass of N is 28.02 g/mol.

The mass of ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is 96.0 g/mol.

Substitute these values in equation (2).

$\begin{aligned}{\text{\% composition of N}} &= \left( {\frac{{{\text{28}}{\text{.02 g/mol}}}}{{{\text{96}}{\text{.0 g/mol}}}}} \right){\text{100 \% }}\\&= {\text{29}}{\text{.1875 \% }} \\ &\approx {\text{2}}{\text{.92 \%}}\\\end{aligned}$

Therefore the percentage composition by mass of nitrogen in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is 29.2 %.

Learn more:

Calculate the moles of chlorine in 8 moles of carbon tetrachloride: link What is the concentration of alcohol in terms of molarity? link

Answer details:

Grade: Senior School

Chapter: Concentration terms

Subject: Chemistry

Keywords: (NH4)2CO3, N, nitrogen, mass, 2.92 %, 96.0 g/mol, 28.02 g/mol, nitrogen, hydrogen, carbon, oxygen, mass of N, mass of (NH4)2CO3.

answered: staxeeyy767

The % composition of nitrogen is 29.166% ~ 29.2%. Thus option 2 is correct.

The percent composition of nitrogen in ammonium carbonate can be calculated as:

% Composition = $\rm \dfrac{mass\;of\;element}{mass\;of\lcompound}\;\times\;100$

Mass of nitrogen in the compound has been:

Number of Nitrogen atoms = 2

Mass of 1 nitrogen atom = 14 g/mol

Mass of 2 nitrogen atom = 28 g/mol

Mass of compound = 96 g/mol

% Composition of nitrogen = $\rm \dfrac{28}{96}\;\times\;100$

% Composition of nitrogen = 29.166 %

The % composition of nitrogen is 29.166% ~ 29.2%. Thus option 2 is correct.

For more information about the percent composition, refer to the link:

link

answered: Guest

idk

explanation:

dasdad

answered: Guest

I’d have to say no because without oxygen in the water the fish would all be dead. so if you want to fish for dead fish, pick the ponds with the lowest oxygen concentrations.