Question

Calculate the number of atoms contained in 5000cm^3 of carbon dioxide gas at room condition​

Answer 1

`\huge\boxed{\sf No.\ of\ atoms = 1.4 * 10^(20) \ atoms}`

Step-by-step explanation:

Given Data:

Volume = v = 5000 cm³ = 0.005 m³

Density of CO₂ at RTP = 1.98 kg / m³

Molar Mass = M = 12 + 16 * 2 = 44 g / mol

Avogadro's No. =
`\sf N_(A)` = 6.023 * 10²³ mol⁻¹

Required:

Number of atoms = ?

Solution:

We know that:

No. of moles (n) = mass in grams / molar mass ∴ Mass = Density * Volume

n = D * v / M

n = 1.98*0.005 / 44

n = 0.000225

Now, Finding the number of atoms

No. of atoms = No. of moles * Avogadro's Number

No. of atoms = 0.000225 * 6.023 * 10²³

No. of atoms = 0.0014 * 10²³

No. of atoms = 1.4 * 10²⁰ atoms

`\rule[225]{225}{2}`

Hope this helped!

~AH1807