How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at 25 $^{o}$ C?
Given: $K_{H}$ of $C O_{2}$ in water $=$ 29.76 atm/(mol/L) at 25 $^{o}$ C

Question

How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at 25

^{o}

C?
Given:

K_{H}

of

C O_{2}

in water

=

29.76 atm/(mol/L) at 25

^{o}

C

Toppr Admin · Accepted Answer

According to Henry-apos-s law- P-KHSS is the solubility in moles per litreKH is the henry-apos-s law constantP is the pressure in atm-Substitute values in the above expression-2-4-29-76-xD7-SS-0-0806MThus 0-0806 moles are present in 1 L of solution- This corresponds to 0-086-xD7-44-3-52g

How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at 25oC?Given: KH of CO2 in water = 29.76 atm/(mol/L) at 25oC3.88 g4.90 g5.33 g3.52 g

According to Henry's law, P=KHSS is the solubility in moles per litreKH is the henry's law constantP is the pressure in atm.Substitute values in the above expression.2.4=29.76×SS=0.0806MThus 0.0806 moles are present in 1 L of solution. This corresponds to 0.086×44=3.52g

How many grams of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at 25 $^{o}$ C?
Given: $K_{H}$ of $C O_{2}$ in water $=$ 29.76 atm/(mol/L) at 25 $^{o}$ C
$3.88$ g
$4.90$ g
$5.33$ g
$3.52$ g