Answer
$NH_3$: $82.27\%$
$CO(NH_2)_2: 46.65\%$
$NH_4NO_3: 35.00\%$
$(NH_4)_2SO_4: 21.20\%$
The compound with highest nitrogen content is $NH_3$, with $82.28\%$
Work Step by Step
$NH_3:$
1. Calculate the molar mass of: $NH_3$
Molar Mass ($NH_3$):
14.01* 1 + 1.008* 3 = 17.03g/mol
2. Calculate the total mass of $N$ in one mole of this compound:
Total Mass ($N$): $ 1 \times 14.01g = 14.01g$
3. Find the mass percent composition:
$\frac{Total-mass (N)}{Molar-Mass} \times 100\% = \frac{ 14.01}{ 17.03} \times 100\% = 82.27\%$
$CO(NH_2)_2$$:$
1. Calculate the molar mass of: $CO(NH_2)_2$
Molar Mass ($CO(NH_2)_2$):
12.01* 1 + 16* 1 + 2 * ( 14.01* 1 + 1.008* 2) = 60.06g/mol
2. Calculate the total mass of $N$ in one mole of this compound:
Total Mass ($N$): $ 2 \times 14.01g = 28.02g$
3. Find the mass percent composition:
$\frac{Total-mass (N)}{Molar-Mass} \times 100\% = \frac{ 28.02}{ 60.06} \times 100\% = 46.65\%$
$NH_4NO_3:$
1. Calculate the molar mass of: $NH_4NO_3$
Molar Mass ($NH_4NO_3$):
14.01* 1 + 1.008* 4 + 14.01* 1 + 16* 3 ) = 80.05g/mol
2. Calculate the total mass of $N$ in one mole of this compound:
Total Mass ($N$): $ 2 \times 14.01g = 28.02g$
3. Find the mass percent composition:
$\frac{Total-mass (N)}{Molar-Mass} \times 100\% = \frac{ 28.02}{ 80.05} \times 100\% = 35.00\%$
$(NH_4)_2SO_4$:
1. Calculate the molar mass of: $(NH_4)_2SO_4$
Molar Mass ($(NH_4)_2SO_4$):
2 * ( 14.01* 1 + 1.008* 4 ) + 32.07* 1 + 16.00* 4 = 132.2g/mol
2. Calculate the total mass of $N$ in one mole of this compound:
Total Mass ($N$): $ 2 \times 14.01g = 28.02g$
3. Find the mass percent composition:
$\frac{Total-mass (N)}{Molar-Mass} \times 100\% = \frac{ 28.02}{ 132.2} \times 100\% = 21.20\%$
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Therefore, the compound with highest nitrogen content is $NH_3$, with $82.28\%$
