The solubility of a gas in a liquid increases with increasing pressure. To under

Question

The solubility of a gas in a liquid increases with increasing pressure.

To understand the above statement, consider a familiar example: cola. In cola and other soft drinks, carbon dioxide gas remains dissolved in solution as long as the can or bottle remains pressurized. As soon as the lid is opened and pressure is released, the CO2 gas is much less soluble and escapes into the air.

The relationship between pressure and the solubility of a gas is expressed by Henry's law: C=kP, where C is concentration in M, k is the Henry's law constant in units of mol/Latm, and P is the pressure in atm.

Note: Since temperature also affects the solubility of a gas in an liquid, the Henry's law constant is specific to a partcular gas at a particular temperature.

The following table provides some information on carbon dioxide solubility in water.

What is the Henry's law constant for CO2 at 20C?

What pressure is required to achieve a CO2 concentration of 5.70×102 M at 20C?

At 1 atm, how many moles of CO2 are released by raising the temperature of 1 liter of water from 20C to 25C?

C
(mol/L) P
(atm) k
(mol/Latm) T
(C) 3.80×102 1.00 20.0 5.70×102 20.0 1.00 3.40×102 25.0

Explanation / Answer

a) let it be x.so,

C=P*k

or 3.8*10^-2 = 1*k

or k=3.8*10^-2 mol/L.atm

b)let the pressure be P.so,

5.7*10^-2=P*3.8*10^-2

or P=1.5 atm

c)solubility at 25C=P*k

=3.4*10^-2 M

so, moles of CO2 released = (3.8-2.4)*10^-2

=0.4*10^-2 moles

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