How many moles of Ne occupy 2.0 L at STP?
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To answer your question, at STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 L. So, if you have 2.0 L of Ne at STP, you would have 2.0/22.4 moles of Ne.
To determine the number of moles of Ne (Neon) occupying 2.0 L at STP (Standard Temperature and Pressure), we will use the ideal gas law. The ideal gas law equation is:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L atm/(mol K))
T = temperature (in Kelvin)
At STP, the pressure is 1 atm, and the temperature is 273.15 K. We can substitute these values into the equation:
PV = nRT
(1 atm) * (2.0 L) = n * (0.0821 L atm/(mol K)) * (273.15 K)
Now, we can solve for the number of moles (n):
2.0 atm L = n * (0.0821 L atm/(mol K)) * (273.15 K)
n = (2.0 atm L) / ((0.0821 L atm/(mol K)) * (273.15 K))
n = 0.0805 moles
Therefore, approximately 0.0805 moles of Ne occupy 2.0 L at STP.
To determine the number of moles of Ne (neon) that occupy 2.0 L at STP (Standard Temperature and Pressure), we can use the Ideal Gas Law equation:
PV = nRT
Where:
- P represents the pressure (which is 1 atm at STP)
- V represents the volume (which is given as 2.0 L)
- n represents the number of moles (the quantity we are trying to find)
- R is the ideal gas constant (0.0821 L·atm/mol·K)
- T represents the temperature
At STP, the temperature is 273.15 K. Now we can rearrange the equation to solve for n:
n = PV / RT
Plugging in the given values:
n = (1 atm) x (2.0 L) / (0.0821 L·atm/mol·K) x (273.15 K)
n = 2.0 / 22.414
n ≈ 0.089 mol
Therefore, approximately 0.089 moles of Ne occupy 2.0 L at STP.