Dinitrogen oxide (N₂O) gas was generated from the thermal decomposition of ammonium nitrate and collected over water. The wet ga
s occupied 130 mL at 21◦C when the atmospheric pressure was 750 Torr. What volume would the same amount of dry dinitrogen oxide have occupied if collected at 750 Torr and 21 ◦C? The vapor pressure of water is 18.65 Torr at 21◦C. Answer in units of mL.
The total pressure of the gas mixture is the sum of the vapor pressure of its constituents. So, the vapor pressure of N₂O(p) can be calculated:
750 = 18.85 + p
p = 750 - 18.85
p = 731.15 torr
It means that for 731.15 torr, N₂O occupied 130 mL. For the general gas equation, we know that
Where <em>p</em> is the pressure, <em>V</em> is the volume, <em>T</em> is the temperature, 1 is the initial state, and 2 the final state. For the same temperatue (21ºC), the equation results on Boyle's law:
Answer:Protons, neutrons, and electrons are the three main subatomic particles found in an atom. Protons have a positive (+) charge. An easy way to remember this is to remember that both proton and positive start with the letter "P." Neutrons have no electrical charge.