Dalton’s law of partial pressures
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In a closed container, the liquid level is at 50% of the container’s volume, and the pressure at this point is 0.1 MPa. If the container is heated to 100 degrees, reaching the saturated vapor pressure of water, how do the partial pressures of the other gases such as oxygen and nitrogen change?
Since it is a closed container, the partial pressures of nitrogen and oxygen each follow the gas law equations, and are independent of the partial pressure of water; whereas the total pressure in the container is related to the partial pressure of water
Can we then approximate that the container pressure will rise to 0.2 MPa?
As the temperature continues to rise, the container will eventually explode.
The total pressure increases, and the partial pressures of nitrogen and oxygen increase as well, but their proportions decrease
Shouldn’t the solubility of gases decrease as temperature rises? In that case, pressure should increase