Part B What pressure is required to achieve a CO2 concentration of 6.90 Solution

Question

Part B What pressure is required to achieve a CO2 concentration of 6.90

Explanation / Answer

You need Henry constant of carbon dioxide at the given temperatures. Henry constant at 25°C =298K is kH(298) = 29.41 L·atm·mol?¹ At other temperatures it can be found using the formula: kH(T) = kH(298)·exp{-C·(1/T - 1/298K) with C = 2400K fo CO2 So at T=20°C=293K kH(293) = 29.41 L·atm·mol?¹·exp{-2400K·(1/293K - 1/298K) = 25.63 L·atm·mol?¹ The answer to the first part can be found directly from Henry's law: p = kH · c = 25.63 L·atm·mol?¹ · 6.9×10?² mol·L?¹ = 1.769atm To find solution of second part, first calculate the concentration in liquid at partial pressure of 1atm and 20°C from Henry's law: p = kH · c => c = p/kH = 1atm / 25.63 L·atm·mol?¹ = 3.90×10?² mol·L?¹ In similar way you can calculate concentration at 25°C c = p/kH = 1atm / 29.41 L·atm·mol?¹ = 3.40×10?² mol·L?¹ So by rising the temperature from 20°C to 25°C the concentration decreases by ?c = 3.90×10?² mol·L?¹ - 3.40×10?² mol·L?¹ = 0.5×10?² mol·L?¹ = 5×10?³ mol·L?¹ Multiply this by the volume of the sample and you get the amount of carbon dioxide released due to temperature rise: n = ?c · V = 5×10?³ mol·L?¹ · 1L = 5×10?³ mol

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