The following table provides some information on carbon dioxide solubility in wa

Question

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

Part A

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

Express your answer in mol L1 bar1 to four decimal places.

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Part B

What pressure is required to achieve a CO2 concentration of 0.0980 mol L1 at 20C?

Express your answer to three significant figures and include the appropriate units.

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Part C

At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20C to 25C?

Express your answer to four decimal places and include the appropriate units.

Sgas
(mol L1) Pgas
(bar) kH
(mol L1 bar1) T
(C) 0.0380 1.01 20.0 0.0980 20.0 1.01 0.0340 25.0

Explanation / Answer

Solution :-

Part A

Given data

Solubility of gas = 0.0380 mol L-1

Pressure of gas = 1.01 bar

KH = ?

Formula to calculate the Henry’s gas constant is as follows

C= KH * p

Where c= concentration of gas (mol L-1)

P = pressure (bar )

Now lets put the values in the formula and calculate the KH

0.0380 mol L-1 = KH * 1.01 bar

0.0380 mol L-1 / 1.01 bar = KH

0.0376 mol L-1 bar-1 = KH

Therefore Henry's law constat KH = 0.0376 mol L-1 bar-1

Part B) Given data

At 20 oC KH= 0.0376 mol L-1 bar-1

C= 0.0980 mol L-1

P = ?

Lets put the values in the formula

C= KH*p

0.0980 mol L-1 = 0.0376 mol L-1 bar-1* p

(0.0980 mol L-1 / 0.0376 mol L-1 bar-1) = p

2.61 bar = p

Therefore pressure needed = 2.61 bar

Part C)

Given data

P = 1.01 bar

KH= 0.0340 mol L-1 bar-1

C= ?

C= KH*p

Lets put the values in the formula

C =0.0340 mol L-1 bar-1 * 1.01 bar

C =0.0343 mol L-1

At 20 oC solubility is 0.0380 mol L- 1 and at 25 oC solubility is 0.0343 mol L-1

So the number of moles of CO2 released = 0.0380 mol – 0.0343 mol

                                                                           = 0.0037 mol CO2

So the number of moles of CO2 released at 25oC = 0.0037 mole CO2

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