Answer:
New Volume = 0.013 Liter
Explanation:
Combined Gas Law Problem
P₁V₁/T₁ = P₂V₂/T₂
P₁ = 1 atm
V₁ = 1.2 Liters
T₁ = 0°C = 273 K
P₂ = 100 atm
V₂ = V₁(P₁/P₂)(T₂/T₁)
T₂ = 15°C = (273 + 15)K = 288K
P₂ = 1.2L(1atm/100atm)(288K/273K) = 0.013 Liter
<h3><u>Answer:</u></h3>
- One mole of gas will occupy the same volume as one mole of any other gas at same temperature and pressure, despite mass difference.
<h3><u>Explanation</u><u>:</u></h3>
The volume occupied by one mole of gas at stp is known as the standard molar volume of a gas. It has been found to be 22.41410 L. According to Avagadro's law, one mole of any gas will occupy the same volume as one mole of any other gas at the same temperature and pressure, despite mass difference. Knowing the volume of gas, you can use 1 mol/22.4L as a conversion factor to find the number of moles, and therefore the mass, of a given volume of a given gas at STP.
<u>Behaviour </u><u>of </u><u>gases:</u>
- In gases, the molecules are far apart and mutual interaction amongst the molecules are negligible except when they collide.
- At low temperature and high pressure, the gases follow a simple reaction:
ㅤㅤㅤ ➝ PV = KT
Its Rhodium....In Period 5 of the Periodic Table.
Phosphorus hope this helps :)
