To solve this problem, we can use the ideal gas law, which states:
PV = nRT
Where:
- P is the pressure in atmospheres (1.8 atm)
- V is the volume in liters (2 L)
- n is the number of moles
- R is the ideal gas constant (0.0821 L atm / (mol K))
- T is the temperature in Kelvin (270 K)
Rearranging the equation to solve for n:
n = PV / RT
Plugging in the given values:
n = (1.8 atm * 2 L) / (0.0821 L atm / (mol K) * 270 K)
n = 3.6 / (0.0821 * 270)
n = 3.6 / 22.167
n ≈ 0.1629 mol
Therefore, there must be approximately 0.1629 moles in a 2L container at 1.8 atmospheres with a temperature of 270K.
Given that R= 0.0821(L atm) / (mol K) how many moles must be in a 2L container at 1.8 atmospheres with a temperature of 270K?
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