How much water would be needed to completely dissolve 1.74 L of the gas at a pressure of 725 torr and a temperature of 18 ∘C?
A gas has a Henry's law constant of 0.192 M/atm .
Answer: Here we have to use the henry's law
C = KP , here , C is concentration , K is henry's constant and P is partial pressure
given mass / molar mass of water* volume = 0.192 * pressure in atm
[ here 1 torr = 0.0013atm hence , 725 torr = 0.95 atm ]
Now , we get : mass / 18 * 1.74 = 0.95 * 0.192
mass = 5.71 gram
Hence the required amount of water is 5.71 gram
How much water would be needed to completely dissolve 1.74 L of the gas at a...
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