Under Henry's law at constant temperature, the dissolved gas concentration changes in what way as gas pressure increases?

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Henry's law says that at a fixed temperature, the amount of gas dissolved in a liquid is proportional to the gas’s partial pressure above the liquid. So the dissolved-gas concentration increases linearly with pressure, following C = kH × P. Double the pressure (within the typical range for dilute solutions) and you roughly double the concentration because the relationship is directly proportional. The proportionality constant kH depends on the specific gas, solvent, and temperature. This is why the correct idea is that concentration increases in direct proportion to pressure. It wouldn’t stay constant, decrease, or rise exponentially under these conditions (exponential would imply a nonlinear relationship not described by Henry’s law; deviations can occur only at very high pressures or non-ideal conditions).