Gas Laws

The Henry's law constant ( ) varies depending on the gas and its temperature. The correct matches are:
- (A) 145 K bar corresponds to CO (I), which has the highest Henry's law constant.
- (B) 89 K bar corresponds to He (II), which is less soluble than CO .
- (C) 76.5 K bar corresponds to N at 293 K (III), as nitrogen is less soluble than CO .
- (D) 1.67 K bar corresponds to N at 303 K (IV), as the solubility of gases decreases with increasing temperature.
Thus, the correct answer is (A)-(I), (B)-(II), (C)-(III), (D)-(IV).

Dalton's law of partial pressures states that the total pressure of a mixture of gases is the sum of the partial pressures of each individual gas in the mixture. Mathematically, this is expressed as: where are the partial pressures of the individual gases. Now let's evaluate each option: - Option (1): — This is the correct expression for Dalton's law when dealing with two gases. - Option (2): — This expression is related to the partial pressure of a gas in terms of its mole fraction ( ) and the vapor pressure of the pure substance ( ). This is a valid expression under Dalton's law for one gas in a mixture. - Option (3): — This is another correct form of Dalton's law that includes partial pressures based on the mole fractions of the gases. It reflects the contributions of two gases to the total pressure. - Option (4): — This is not a valid expression according to Dalton's law. This suggests that the partial pressure of gas 1 is the total pressure minus the partial pressure of gas 2, which does not accurately reflect Dalton's law.
Thus, the correct answer is Option (4), as it does not properly represent Dalton's law.

The given equation is p = K_Hx, which represents Henry's Law in chemistry. In this expression:

Step 1: Understanding deviation from ideal behavior.
Gases deviate from ideal behavior due to intermolecular forces and the volume occupied by the gas molecules. At high pressure, these deviations become more significant.
Step 2: Analyze intermolecular forces.
Hydrogen and Helium are light and exhibit very weak intermolecular forces.
Neon, a noble gas, also has weak van der Waals forces.
Carbon dioxide, being a larger and more polarizable molecule, has stronger intermolecular attractions, leading to greater deviation.
Step 3: Conclusion.
At high pressure, Carbon dioxide deviates the most from ideal gas behavior due to its significant van der Waals forces and molecular size.