Which among the following gases exhibits very low solubility in water at room temperature?

Which of the following statements is correct?

How many grams of carbon dioxide gas are dissolved in $1 \ L$ of carbonated water,if the manufacturer uses a pressure of $2.4 \ atm$ in the bottling process at $25^{\circ} C$ (in $g$)? ($K_{H}$ of $CO_2 = 3000 \ atm$)

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.

Air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportions of $20\%$ and $79\%$ by volume at $298\ K$. The water is in equilibrium with air at a pressure of $10\ atm$. At $298\ K$,if the Henry's law constants for oxygen and nitrogen are $3.30 \times 10^7\ mm$ and $6.51 \times 10^7\ mm$,respectively,the mole ratio of gases $(O_2 : N_2)$ dissolved in water is about

Which of the following statements is $NOT$ true about solubility?