Advertisements
Advertisements
Question
Henry’s law constant for CO2 in water is 1.67 × 108 Pa at 298 K. Calculate the quantity of CO2 in 500 mL of soda water when packed under 2.5 atm CO2 pressure at 298 K.
Solution
Given, KH = 1.67 × 108 Pa
`"P"_("CO"_2)` = 2.5 atm = 2.5 × 101325 Pa
According to Henry’s law,
`"P"_("CO"_2) = "K"_"H" xx "x"_("CO"_2)`
∴ `"x"_("CO"_2) = "P"_("CO"_2)/"K"_"H"`
= `(2.5 xx 101325 "Pa")/(1.67 xx 10^8 "Pa")`
= 1.517 × 10−3
We can write, `"x"_("CO"_2) = ("n"_("CO"_2))/("n"_("CO"_2) + "n"_("H"_2"O")) = ("n"_("CO"_2))/("n"_("H"_2"O")) = 1.517 × 10^(−3) ...["Since, n"_("CO"_2) "is negligible as compared to n"_("H"_2"O")]`
For 500 mL of soda water, the volume of water = 500 mL; the mass of water = 500 g,
We can write:
= `500/18 "mol of water"`
= 27.78 mol of water
i.e., `"n"_("H"_2"O")` = 27.78
∴ `("n"_("CO"_2))/"n"_("H"_2"O") = "x"_("CO"_2)`
`("n"_("CO"_2))/(27.78) = 1.517 xx 10^(−3)`
or `"n"_("CO"_2)` = 42.14 × 10−3 mole
Mass of CO2 = 42.14 × 10−3 × 44 g = 1.854 g
APPEARS IN
RELATED QUESTIONS
What is the effect of temperature on solubility of a gas in a liquid?
Gas (A) is more soluble in water than Gas (B) at the same temperature. Which one of the two gases will have the higher value of KH (Henry’s constant) and why
State Henry’s law.
H2S, a toxic gas with rotten egg like smell, is used for the qualitative analysis. If the solubility of H2S in water at STP is 0.195 m, calculate Henry’s law constant.
The partial pressure of ethane over a solution containing 6.56 × 10−3 g of ethane is 1 bar. If the solution contains 5.00 × 10−2 g of ethane, then what shall be the partial pressure of the gas?
Based on solute-solvent interactions, arrange the following in order of increasing solubility in n-octane and explain.
Cyclohexane, KCl, CH3OH, CH3CN
The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen are 3.30 × 107 mm and 6.51 × 107 mm respectively, calculate the composition of these gases in water.
How does solubility of a gas in water varies with the temperature?
State Henry's Law. What is the effect of temperature on the solubility of a gas in a liquid?
The solubility product of PbCl2 at 298K is 1.7 × 10-5. Calculate the solubility of PbCl2 in g/lit. at 298K.
Atomic Weights: [Pb = 207 and Cl = 35.5]
Which law shows relation between pressure and solubility of a gas in solvent?
The value of Henry's constant KH is ______.
Which of the following factor(s) affect the solubility of a gaseous solute in the fixed volume of liquid solvent?
(a) nature of solute
(b) temperature
(c) pressure
(i) (a) and (c) at constant T
(ii) (a) and (b) at constant P
(iii) (b) and (c) only
(iv) (c) only
KH value for \[\ce{Ar(g)}\], \[\ce{CO2(g)}\], \[\ce{HCHO (g)}\] and \[\ce{CH4(g)}\] are 40.39, 1.67, 1.83 × 10–5 and 0.413 respectively. Arrange these gases in the order of their increasing solubility.
The solubility of a gas in water depends on ______
Assume that argon exerts a partial pressure of 6 bar. Calculate the solubility of argon gas in water. (Given Henry’s law constant for argon dissolved in water, KH = 40 k bar)
If O2 gas is bubbled through water at 303 K, the number of millimoles of O2 gas that dissolve in 1 litre of water is ______. (Nearest integer)
(Given: Henry's Law constant for O2 at 303 K is 46.82 k bar and partial pressure of O2 = 0.920 bar)
(Assume solubility of O2 in water is too small, nearly negligible)
Identify that the following compound is insoluble, partially soluble and highly soluble in water.
ethylene glycol
