560 mL of Xe will equal how many moles @ STP?
To determine the number of moles of Xe at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (STP is 1 atmosphere, or 1 atm)
V = Volume (560 mL)
n = Number of moles (what we are trying to find)
R = Ideal gas constant (0.0821 L∙atm/mol∙K)
T = Temperature (STP is 273.15 K)
First, we need to convert the volume from milliliters (mL) to liters (L), since the ideal gas law requires volume in liters:
1 L = 1000 mL
So, 560 mL = 560/1000 = 0.56 L
Now we can substitute the known values into the equation:
(1 atm) * (0.56 L) = n * (0.0821 L∙atm/mol∙K) * (273.15 K)
Simplifying the equation:
0.56 = n * (0.0821 * 273.15)
0.56 = n * 22.41471515
Dividing both sides by 22.41471515 to solve for n:
n = 0.56 / 22.41471515
n ≈ 0.025 moles
Therefore, 560 mL of Xe at STP is approximately equal to 0.025 moles.