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Byju's Answer

Standard XII

Chemistry

Faraday's First Law

How many gram...

Question

How many grams of $C O_{2}$ gas is dissolved in a $1 l i t r e$ bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at $25^{o} C ? ($ given $K_{H}$ of $C O_{2}$ water $= 9.6 a t m / m o l / l$ at $25^{o} C$ )

0.25

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0.27

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Solution

The correct option is C 11
Henry’s Law states that, $P = K_{H} S$

$P$ is the pressure in atm

$K_{H}$ is the Henry’s law constant,

$S$ is the solubility in moles per litre

Putting all the values in equation;

$2.4 = 9.6 \times S$

$S = 0.25$ mol/lit

Mass of $C O_{2}$ dissolved $= 0.25 \times 44 = 11$ g

Hence option C is correct.

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Similar questions

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K_{H}

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= 29.76 a t m / m o l e / l

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How many grams of CO2 gas is dissolved in a 1 litre bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at 25oC?( given KH of CO2 water =9.6atm/mol/l at 25oC)

The correct option is C 11Henry’s Law states that, P=KHS P is the pressure in atm KH is the Henry’s law constant, S is the solubility in moles per litre Putting all the values in equation; 2.4=9.6×S S=0.25 mol/lit Mass of CO2 dissolved =0.25×44=11g Hence option C is correct.

How many grams of $C O_{2}$ gas is dissolved in a $1 l i t r e$ bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at $25^{o} C ? ($ given $K_{H}$ of $C O_{2}$ water $= 9.6 a t m / m o l / l$ at $25^{o} C$ )