In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
it stays the same
No, it will not condense if its partial pressure does not exceed its (maximum) partial pressure of the component's liquid (or solution) at the same(!) temperature.
Pressures simply add. If the partial pressure of gas is three and the partial pressure of water is five, the total pressure is eight. Find the partial pressure for water at the temperature of your experiment, subtract it from your pressure reading. As an aside, if you've corked your glassware rather than using a slider or a water bath, expect stupid results.
The pressure of each gas in a mixture is called the partial pressure of that gas.
From Wikipedia, article "relative humidity": "It is defined as the ratio of the partial pressure of water vapor in the air-water mixture to the saturated vapor pressure of water at the prescribed temperature." So, you somehow measure the partial pressure of water vapor, look up the saturated vapor pressure of water for the current temperature, and take the ratio.
Yes. If the pressure is increased, even with a noble gas, the reaction equilibrium will shift to alleviate and lower that increased pressure (if there are more moles of gas on one side of the reaction than the other).
The total pressure will be 5 atm and the partial pressure of gas 1 will be 2 atm and the partial pressure of gas 2 will be 3 atm.
When air pressure is Low it becomes very difficult to breath simply because air moves from high partial pressure to low partial pressure.
vapor pressure
No, it will not condense if its partial pressure does not exceed its (maximum) partial pressure of the component's liquid (or solution) at the same(!) temperature.
The higher the pressure, the more easily a chemical diffuses. And seeing as pressure and temperature are directly related, the higher the temperature the more easily a chemical diffuses, and vice versa. This is caused by everything "wanting" to be equal, if there is a higher pressure, then it will diffuse to an area of lower pressure.
Pressures simply add. If the partial pressure of gas is three and the partial pressure of water is five, the total pressure is eight. Find the partial pressure for water at the temperature of your experiment, subtract it from your pressure reading. As an aside, if you've corked your glassware rather than using a slider or a water bath, expect stupid results.
Rate of diffusion will increase.
The pressure of each gas in a mixture is called the partial pressure of that gas.
Decreases. Delta S will be negative since 2 mol of gaseous reactants form 1 mol of gaseous product.
The partial pressure is the pressure exerted by just one gas in the mixture.
From Wikipedia, article "relative humidity": "It is defined as the ratio of the partial pressure of water vapor in the air-water mixture to the saturated vapor pressure of water at the prescribed temperature." So, you somehow measure the partial pressure of water vapor, look up the saturated vapor pressure of water for the current temperature, and take the ratio.
The partial pressure is the pressure exerted by just one gas in the mixture.