The relationship between pressure and the solubility of a gas is expressed by He

Question

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

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

2.What pressure is required to achieve a CO2 concentration of 6.60×102 M at 20C?

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

Please show all work

Thank you!

Explanation / Answer

Henry's law expression is s = kP

1) Given S = 3.7x 10-2 mol/L and P = 1 atm

Thus k = S/P = 3.7x 10-2 mol/L /1 atm

= 3.7x 10-2 mol/L .atm

Henry's constatn at 20 C is 3.7x 10-2 mol/L .atm

b) Now S = 6.6x10-2 M = 6.6x10-2 mol/L

thus P = S/k = 6.6x10-2 M / 3.7x10-2 M/atm

P = 1.7838 atm

c) Now the solubility of gas at 25C is

S = kP

Given k = 3.4 x10-2 mol/L.atm and P = 1 atm

Then S = 3.4 x10-2 mol/L.atm /1 atm

=3.4 x10-2 mol/L

The moles of gas liberated from one L of solution on heating from 20 to 25 C is

= S at 20 C - Sat 25 C

= 3.7 x10-2 moles - 3.4x10-2 moles in one L solution

= 0.3x10-2

= 3.0x10-3 moles are expelled from one litre of solution on heating.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.