A gas occupies 4.69 L when the temperature is 45.0oC and at 1.05 atm of pressure. What temperature change (in K) will be needed to change the volume to 6.15 L at constant pressure? Report your answer to 3 significant figures and do not include units in your answer.
At what temperature (in oC) does 11.41 g of neon occupy a volume of 11.49 L at a pressure of 1.41 atm? Report your answer to 3 significant figures and do not include units in your answer.
At a fixed temperature, equal moles of SO2 (g) and O2 (g) are mixed in a constant pressure container (the volume of the container changes in order to keep the pressure at a constant value). The SO2 (g) and O2 (g) are allowed to react, producing SO3 (g):2 SO2 (g) + O2 (g) → 2 SO3 (g)
If the initial volume of the container, before any reaction takes place, is 2.00 L, determine the volume of the container after the SO2 (g) and O2 (g) have reacted to completion.
The final volume will be L
Calculate the density of Xe (g), in g/L, at STP to three significant figures.
Mixtures of helium and oxygen are used in scuba diving tanks to help prevent "the bends". For a particular dive, 21.2 L of oxygen gas at 25.0oC and 1.77 atm, and 6.21 L of helium gas at 25.0oC and 1.3 atm were pumped into a tank with a volume of 6.00 L at 25.0oC.
Calculate (in atm):
1. the partial pressure of oxygen
2. the partial pressure of helium
3. the total pressure in the tank at 25.0oC.