JEE MAIN - Chemistry (2019 - 9th January Morning Slot - No. 10)
Which one of the following statements regarding Henry's law is not correct ?
Higher the value of KH at a given pressure, higher is the solubility of the gas in the liquids
Different gases have different KH (Henry's law constant) values at the same temperature.
The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.
The value of KH increases with increase of temperature and KH is function of the nature of the gas
Explanation
From Henry's law we know,
Pgas = KH xg
Where, Pgas = Pressure of undissolved gas
xg = Mole fraction of gas dissolved into the liquid.
KH = Henry's Carnot.
When pressure is constant then,
xg $$ \propto $$ $${1 \over {K{}_H}}$$
So. when KH is high then xg or solubility of gas is lower in the liquid.
So, option (A) is wrong.
Pgas = KH xg
Where, Pgas = Pressure of undissolved gas
xg = Mole fraction of gas dissolved into the liquid.
KH = Henry's Carnot.
When pressure is constant then,
xg $$ \propto $$ $${1 \over {K{}_H}}$$
So. when KH is high then xg or solubility of gas is lower in the liquid.
So, option (A) is wrong.
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