What is the relation between Kh ( Henry's law constant) and molecular weight?

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Q. Solubility of a gas X in liquid Y is given by Henry's law written as

P = K_{H} \times x

. Where

K_{H}

is Henry constant, P is partial pressure of the gas and x is mole fraction of gas in liquid. Which of the following is incorrect about

K_{H} -

Henrys law constant $[K_{H}]$ for four gases at 293 K are,

$H e [144.97 K b a r], H_{2} [69.16 K b a r], N_{2} [76.48 K b a r], O_{2} [34.86 K b a r]$ .

Which gas is more soluble in water at a given pressure.

Q. Solubility of a gas X in liquid Y is given by Henry's law written as

P = K_{H} \times x

. Where

K_{H}

is Henry constant, P is partial pressure of the gas and x is mole fraction of gas in liquid. Which of the following is incorrect about

K_{H} -

In Boyles law experiment the graph drawn between pressure and density for a given temperature of different gases are the straight lines then the molecular weights have the relation

Q. If for hydrogen

C_{p} - C_{v} = m

and for nitrogen

C_{p} - C_{v} = n

, where

C_{p}

and

C_{v}

refer to specific heats per unit mass respectively at constant pressure and constant volume, the relation between

m

and

n

is (molecular weight of hydrogen

= 2

and molecular weight of nitrogen

= 14

)

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