You visited us 10 times! Enjoying our articles? Unlock Full Access!

Relative Lowering of Vapour Pressure

The elevation...

Question

The elevation in boiling point of a solution of 13.44 g of $C u C l_{2}$ (Molar mass 134.4) in 1 kg water is:
$[K_{b} = 0.52$ K molality $^{- 1}]$

0.16

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

0.05

No worries! We‘ve got your back. Try BYJU‘S free classes today!

0.1

No worries! We‘ve got your back. Try BYJU‘S free classes today!

0.2

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $0.16$
The elevation in boiling point of a solution is 0.16
$Δ T_{b} = i K_{f} m$
$Δ T_{b} = \frac{1000 \times 0.52 \times 13.44}{134.4 \times 1000} (1 + 2 α)$
$∴ Δ T_{b} = 0.156 (∵ α = 1)$

Hence, the correct option is $A$

Suggest Corrections

Similar questions

Q. The elevation in boiling point of a solution of

13.44 g

C u C l_{2}

in 1 kg of water using the following information will be ( Molecular weight of

C u C l_{2} = 134.4

and

K_{b} = 0.52 K m o l a l^{- 1}

Q. The elevation in boiling point of a solution of 13.44 g of

C u C l_{2}

(Molar mass 134.4) in 1 kg water is:

[K_{b} = 0.52 K {molality}^{- 1}]

The elevation in boiling point of a solution of 13.44g of CuCl₂ in 1kg of water using the following information will be (Molecular weight of CuCl₂= 134.4 and K_b= 0.52K molal^-1)

Q. The elevation in boiling point of a solution of

13.44 g

{C u C l}_{2}

, (molecular weight

= 134.4

K_{b} =

0.52 K molarity ) in 1 kg water using the following information will be:

Q. What will be the elevation in boiling point for

13.44 g

C u C l_{2}

dissolved in

1 k g

of water as solvent if

C u C l_{2}

is fully ionised?
(

K_{b} = 0.52 K k g m o l^{- 1}

Molar mass of

C u C l_{2} = 134.4 g / m o l

)

Join BYJU'S Learning Program

The elevation in boiling point of a solution of 13.44 g of CuCl2 (Molar mass 134.4) in 1 kg water is:[Kb=0.52 K molality−1]

The correct option is A 0.16The elevation in boiling point of a solution is 0.16ΔTb=iKfmΔTb=1000×0.52×13.44134.4×1000(1+2α)∴ΔTb=0.156(∵α=1)Hence, the correct option is A

The elevation in boiling point of a solution of 13.44 g of $C u C l_{2}$ (Molar mass 134.4) in 1 kg water is:
$[K_{b} = 0.52$ K molality $^{- 1}]$

The correct option is A $0.16$
The elevation in boiling point of a solution is 0.16
$Δ T_{b} = i K_{f} m$
$Δ T_{b} = \frac{1000 \times 0.52 \times 13.44}{134.4 \times 1000} (1 + 2 α)$
$∴ Δ T_{b} = 0.156 (∵ α = 1)$

Hence, the correct option is $A$