Choose the correct statement.

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(C) Among the given statements,only statement $(c)$ is correct regarding the Henry's law constant $(K_{H})$.$(a)$ $K_{H}$ is a function of the nature

Vedclass · Accepted Answer

$K_{H}$ value increases on increasing the temperature of the solution.

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(C) Among the given statements,only statement $(c)$ is correct regarding the Henry's law constant $(K_{H})$.$(a)$ $K_{H}$ is a function of the nature of the gas and the solvent used; therefore,the $K_{H}$ value is not the same for a gas in different solutions.$(b)$ According to Henry's law,$p = K_{H} \cdot x$,which implies $x = p / K_{H}$. Thus,a higher $K_{H}$ value corresponds to lower solubility of the gas.$(c)$ $K_{H}$ is temperature-dependent and generally increases with an increase in temperature,which explains why gases are less soluble in warm water.$(d)$ Easily liquefiable gases have stronger intermolecular forces,which leads to lower $K_{H}$ values.

Similar Questions

If $N_2$ gas is bubbled through water at $293 \ K$,how many millimoles of $N_2$ gas would dissolve in $1 \ L$ of water? Assume that $N_2$ exerts a partial pressure of $0.987 \ bar$. Given that Henry's law constant for $N_2$ at $293 \ K$ is $76.48 \ kbar$.

Which one of the following statements regarding Henry's law is not correct?

The statement “If $0.003 \ mol$ of a gas are dissolved in $900 \ g$ of water under a pressure of $1 \ atm$,$0.006 \ mol$ will be dissolved under a pressure of $2 \ atm$”,illustrates:

Calculate the solubility of a gas in a solvent at a pressure of $3 \text{ atm}$ and $25 \text{ }^\circ\text{C}$. (Given: Henry's law constant $K_H = 3.0 \times 10^{-2} \text{ mol dm}^{-3} \text{ atm}^{-1}$) (in $\text{ M}$)

Assertion $(A)$: For an endothermic dissolution process,an increase in temperature increases the solubility in a nearly saturated solution.
Reason $(R)$: In a saturated solution,dynamic equilibrium exists between the dissolved solute and the undissolved solute.

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