Find the Density at STP NH_3O_3I

$N H_{3} O_{3} I$

Step 1

To find the mass of $1$ mole of $N H_{3} O_{3} I$ look up the atomic mass of each element and multiply it by the number of atoms contained in each element in the molecule.

mass of $1$ mole of $N H_{3} O_{3} I$ $=$ $(mass of N)$ + $3 (mass of H)$ + $3 (mass of O)$ + $(mass of I)$

Step 2

Fill in the atomic masses from the periodic table.

mass of $1$ mole of $N H_{3} O_{3} I$ $=$ $(14.01000022)$ + $3 (1.00999999)$ + $3 (16)$ + $(126.90000152)$

Step 3

Simplify the result.

Remove parentheses.

mass of $1$ mole of $N H_{3} O_{3} I = (14.01000022) + 3 (1.00999999) + 3 (16) + 126.90000152 g$

Simplify each term.

Multiply $3$ by $1.00999999$ .

mass of $1$ mole of $N H_{3} O_{3} I = 14.01000022 + 3.02999997 + 3 (16) + 126.90000152 g$

Multiply $3$ by $16$ .

mass of $1$ mole of $N H_{3} O_{3} I = 14.01000022 + 3.02999997 + 48 + 126.90000152 g$

Simplify by adding numbers.

Add $14.01000022$ and $3.02999997$ .

mass of $1$ mole of $N H_{3} O_{3} I = 17.0400002 + 48 + 126.90000152 g$

Add $17.0400002$ and $48$ .

mass of $1$ mole of $N H_{3} O_{3} I = 65.0400002 + 126.90000152 g$

Add $65.0400002$ and $126.90000152$ .

mass of $1$ mole of $N H_{3} O_{3} I = 191.94000172 g$

Step 4

One mole of any gas occupies $22.4 L$ at STP (standard temperature and pressure).

$V = 22.4 L$

Step 5

Density is mass over volume.

$\frac{191.94000172 g}{22.4 L}$

Step 6

Factor $191.94000172$ out of $191.94000172 g$ .

$\frac{191.94000172 (g)}{22.4 L}$

Step 7

Factor $22.4$ out of $22.4 L$ .

$\frac{191.94000172 (g)}{22.4 (L)}$

Step 8

Separate fractions.

$\frac{191.94000172}{22.4} \cdot \frac{g}{L}$

Step 9

Divide $191.94000172$ by $22.4$ .

$8.56875007 \frac{g}{L}$

Step 10

Combine $8.56875007$ and $\frac{g}{L}$ .

$\frac{8.56875007 g}{L}$

Find the Density at STP NH_3O_3I

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