More gas dissolves into the liquid.
The solubility of a gas in a liquid increases as the pressure increases.
Solubility and pressure share a direct relationship. In other words, as pressure goes up, solubility goes up, and vice versa. This is known as Henry's Law. It is shown by the formula: S1/P1=S2/P2
the solubility of gas increases as pressure increases
When pressure increases, the solubility of a gas in a liquid will increase.
Increasing the pressure increases the solubility of a gas.
When pressure increases, the solubility of a gas also increases.
The boiling point of a liquid increases when atmospheric pressure is increased.
If the temperature of the liquid is raised, more molecules escape to the vapor until equilibrium is once again established. The vapor pressure of a liquid, therefore, increases with increasing temperature.
It evaporates :)
An aqueous solution has 0.0070 gram of oxygen dissolved in 1000. grams of water. calculate the dissolved oxygen concentration of this solution in parts per million?A. 17ppm B. 27ppm C. 7ppm D. 7ppm
These factors are temperature and pressure.
More gas dissolves into the liquid.
It heats up and precipitates out solids.
The boiling temperature of a liquid increases as the gas pressure a the liquid's surface increases.
The boiling point of a liquid increases when atmospheric pressure is increased.
There is so much pressure that the hydrogen gas gets turned into a liquid, a metallic state.
If the temperature of the liquid is raised, more molecules escape to the vapor until equilibrium is once again established. The vapor pressure of a liquid, therefore, increases with increasing temperature.
A liquid in which something has been dissolved is usually referred to as a 'solution'.
I'm not 100% sure that "solubility" is the right word to use here, but the amount of dissolved gas in a liquid will decrease as the partial pressure of the gas above the liquid decreases.Basically The solubility decreases.
Henry's law states that the solubility of a gas is directly proportional to the partial pressure of that gas over the liquid. The higher the partial pressure, the more gas will be dissolved-- that's why your blood boils in a vacuum; there's not enough pressure to keep the gas in it dissolved.
Henry's law states that the solubility of a gas is directly proportional to the partial pressure of that gas over the liquid. The higher the partial pressure, the more gas will be dissolved-- that's why your blood boils in a vacuum; there's not enough pressure to keep the gas in it dissolved.
As the temperature of a liquid decreases the amount of gas that can be dissolved increases.
Henry's law states that the solubility of a gas is directly proportional to the partial pressure of that gas over the liquid. The higher the partial pressure, the more gas will be dissolved-- that's why your blood boils in a vacuum; there's not enough pressure to keep the gas in it dissolved.