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?
What's wrong with substituting the numbers into
PV = nRT and solving for n?
idk thats just the question, i dont understand it
To find the number of moles in a 2L container at 1.8 atmospheres and 270K, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = gas constant (0.0821 L⋅atm / mol⋅K)
T = temperature (in Kelvin)
We can rearrange this equation to solve for n:
n = PV / (RT)
Now let's substitute the given values into the equation:
P = 1.8 atm
V = 2 L
R = 0.0821 L⋅atm / (mol⋅K)
T = 270 K
n = (1.8 atm x 2 L) / (0.0821 L⋅atm / (mol⋅K) x 270 K)
Simplifying:
n = 3.6 / (22.203 L⋅mol / K)
n = 0.16267 mol
Therefore, there must be approximately 0.16267 moles of gas in a 2L container at 1.8 atmospheres and 270K.
To find the number of moles in a 2L container at 1.8 atmospheres and 270K, we can use the ideal gas law equation:
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)
Rearranging the equation to solve for n:
n = PV / RT
Plugging in the given values:
P = 1.8 atmospheres
V = 2 liters
R = 0.0821 L⋅atm/(mol⋅K)
T = 270K
n = (1.8 atm * 2 L) / (0.0821 L⋅atm/(mol⋅K) * 270K)
Now we can solve this equation:
n = 3.6 / (0.0821 * 270)
n ≈ 0.170 moles
Therefore, there must be approximately 0.170 moles in a 2L container at 1.8 atmospheres and 270K.