Henry's law for the solubility of a gas in a liquid is best stated as:

Henry's law: $p = K_H x$, where $p$ is the partial pressure of the gas above the solution, $x$ is the mole fraction of the dissolved gas, and $K_H$ is the Henry's law constant. A larger $K_H$ for a given $p$ means a smaller $x$, so a larger $K_H$ corresponds to *lower* solubility — the OCR's mention of 'greater $K_H$ greater solubility' is misleading. Solubility of a gas decreases with rising temperature.