How much water would be needed to completely dissolve 1.78 L of the gas at a pressure of 735 torr and a temperature of 24 ∘C?

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Chemistry

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24 December, 19:07

How much water would be needed to completely dissolve 1.78 L of the gas at a pressure of 735 torr and a temperature of 24 ∘C?

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Agustin Hodge · Answer 1

Answer: 0.46L

Explanation:

KH = 0.158mol/L/atm

Pg = 735 torr = 735/760 = 0.967atm

C=?

C = KH x Pg = 0.158 x 0967

C = 0.153mol/L

T = 24°C = 24 + 273 = 297K

R = 0.082atm. L/K/mol

P = 0.967atm

V = 1.78 L

n=?

PV = nRT

n = PV / RT = (0.967x1.78) / (0.082x297)

n = 0.071mol

0.153mol dissolves in 1L of water. therefore, 0.071mol will dissolve in = 0.071/0.153 = 0.46L