The boiling point of solution containing 2.62 g of substance A in 100 g of water is higher by 0.0512°C than the boiling point of pure water. The molar mass of substance is
Answers
The molar mass of the given substance is 266.093 g grams
- In this question, we will use the formula for the elevation of boiling point which comes under colligative properties of solutions.
- The formula to be used is:
ΔT = Kᵇm
ΔT = Kᵇ × 1000 × w₂ / M₂ × w₁
Where,
ΔT= Elevation in boiling point = 0.0512°C
Kᵇ = Ebullioscopic constant
w₁ = mass of solvent = 100g
w₂ = mass of solute = 2.62g
M₂= molar mass of solute
Kᵇ of water = 0.52 K kg mol-1
M₂ = Kᵇ × 1000 × w₂ / ΔT × w₁ = 0.52× 1000 × 2.62 / 0.0512 × 100 = 266.093 g
Thus, according to the calculations, the molar mass of substance A will be 266.093 grams.
Answer:
The molar mass of the given
substance is 266.093 g grams
In this question, we will use the formula for the elevation of boiling point which comes under colligative properties of solutions.
• The formula to be used is:
AT = Kbm
AT = Kb x 1000 × W₂/
M₂ x W₁
Where,
AT= Elevation in boiling point = 0.0512°C
Kb = Ebullioscopic constant
W₁ = mass of solvent = 100g
W₂ = mass of solute = 2.62g
M₂= molar mass of solute
Kb of water = 0.52 K kg mol-1
M₂ = Kb × 1000 × W₂/AT x W₁ = 0.52x 1000 x 2.62 / 0.0512 x 100 = 266.093 g
Thus, according to the calculations, the molar mass of substance A will be 266.093 grams.
Explanation: