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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

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0.05

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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 $A$

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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

)

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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 $A$