MHT CET · Chemistry · Solutions
Regarding to Henry's law which of the following is not correct statement?
- A Different gases have different \(K_H\) (Henry's law constant) values at the same temperature
- B The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution
- C Higher the value of \(\mathrm{K}_{\mathrm{H}}\) at a given pressure, higher is the solubility of the gas in the liquids
- D The value of \(K_H\) increases with increase of temperature and \(K_H\) is function of the nature of the gas
Answer & Solution
Correct Answer
(C) Higher the value of \(\mathrm{K}_{\mathrm{H}}\) at a given pressure, higher is the solubility of the gas in the liquids
Step-by-step Solution
Detailed explanation
\(
\mathrm{p}=\mathrm{K}_{\mathrm{H}} \times \mathrm{x}
\)
Where \(K_H=\) Henry law constant
Henry's constant increases with increase in temperature while it decreases with increase in solubility. Hence, value of \(K_H\)
increases as solubility of gas increases is a wrong statement.
\mathrm{p}=\mathrm{K}_{\mathrm{H}} \times \mathrm{x}
\)
Where \(K_H=\) Henry law constant
Henry's constant increases with increase in temperature while it decreases with increase in solubility. Hence, value of \(K_H\)
increases as solubility of gas increases is a wrong statement.
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