A sample of pure ammonia gas (\text{NH}_3) has a mass of 3.4\text{ g}. What is the total n… — JAMB UTME

A sample of pure ammonia gas ( $\text{NH}_3$ ) has a mass of $3.4\text{ g}$ . What is the total number of atoms contained in this sample? $[\text{N} = 14, \text{H} = 1, N_A = 6.02 \times 10^{23}\text{ mol}^{-1}]$

$4.816 \times 10^{23}$ Cevap
B
$1.204 \times 10^{23}$
C
$3.612 \times 10^{23}$
D
$2.408 \times 10^{23}$

Cevap

4.816 \times 10^{23}

atoms

The molar mass of ammonia (

\text{NH}_3

) is

17\text{ g/mol}

. A mass of

3.4\text{ g}

corresponds to

0.2\text{ moles}

\text{NH}_3

molecules, which contains

1.204 \times 10^{23}

molecules. Because one molecule of

\text{NH}_3

consists of

4

atoms (

1

nitrogen atom and

3

hydrogen atoms), multiplying

1.204 \times 10^{23}

4

gives

4.816 \times 10^{23}

total atoms.

Adım Adım Çözüm

Calculate the molar mass of ammonia (

\text{NH}_3

)

\text{Molar Mass} = 14 + 3(1) = 17\text{ g/mol}

Molar mass is required to convert sample mass into moles.

Calculate the number of moles of

\text{NH}_3

\text{Moles} = \frac{3.4\text{ g}}{17\text{ g/mol}} = 0.2\text{ mol}

Dividing given mass by molar mass yields the mole quantity.

Determine the number of molecules of

\text{NH}_3

\text{Molecules} = 0.2\text{ mol} \times 6.02 \times 10^{23}\text{ mol}^{-1} = 1.204 \times 10^{23}\text{ molecules}

Multiplying moles by Avogadro's constant gives total molecules.

Calculate the total number of individual atoms

\text{Total atoms} = 1.204 \times 10^{23} \times 4 = 4.816 \times 10^{23}\text{ atoms}

Each

\text{NH}_3

molecule contains 1 nitrogen atom and 3 hydrogen atoms (4 atoms in total).

Anahtar Kavram

Converting mass to number of constituent atoms using Avogadro's constant and molecular stoichiometry.

Soru

Cevap

Adım Adım Çözüm

Anahtar Kavram

Sık Yapılan Hatalar

Konular

Bu konudan daha fazla soru