Before moving onto analyzing some examples, here are few reminders.📝

Example 1👇​

What is the number of moles of methane in 1.44 dm³ of the gas measured at room temperature and pressure?

(Molar Volume of gas at room temperature and pressure= 24 dm³mol^-1)

Answer: No of moles of methane= Volume of methane/Molar volume of gas

Example 2👇​

What is the volume, measured at room temperature and pressure, occupied by 13.2 g of carbon dioxide?

(Relative atomic masses: C=12, O=16; Molar Volume of gas at room temperature and pressure= 24 dm³mol^-1 )

Step 1: Find the moles of CO₂

Thus, moles of CO₂ = 13.2 g / (12+16+16) = 0.300 mol

💪​Final Step: Rearrange the formula to find the volume of gas

Volume of CO ₂= 0.300 mol × 24 dm³mol^-1 = 7.20 dm³

Example 3👇​​

Butane burns in oxygen completely to produce carbon dioxide and water according to the following equation:

2C₄H₁₀(g) + 13O₂(g) ⇒ 8CO₂(g) + 10H₂O(l)

What volume of oxygen is needed for the complete combustion of butane measured at room temperature and pressure?

(Molar Volume of gas at room temperature and pressure= 24 dm³mol^-1= 24000 cm³ mol^-1)

Step 1: Find the moles of C₄H₁₀ using the formula

Moles of C₄H₁₀= Volume of C₄H₁₀/ Molar Volume of gas

Hence, 480 cm³/ 24000 cm³mol^-1=0.02 mol

Step 2: Use mole ratio to find the moles of O₂

Moles of O₂ = 0.02 × (13/2) = 0.130 mol

💪​Last Step: Rearrange the formula to find the volume of O₂

Volume of O₂ = 0.130 mol × 24 dm³mol^-1 = 3.12 dm³

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