How many moles of methane occupy a volume of 2.00 L at 50.0 degrees C and 0.500 atm? What formula do I use and how do I get it to moles??
PV=nRT
n= PR/RT
0.0377
To calculate the number of moles of methane, you can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
First, you need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 50.0 + 273.15 = 323.15 K
Now, rearrange the Ideal Gas Law equation to solve for n:
n = (PV) / (RT)
Plugging in the values:
P = 0.500 atm
V = 2.00 L
R = 0.0821 L.atm/mol.K
T = 323.15 K
n = (0.500 atm * 2.00 L) / (0.0821 L.atm/mol.K * 323.15 K)
Calculating this will give you the number of moles of methane.
To calculate the number of moles of methane, you 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)
However, before applying the ideal gas law, you need to convert the temperature from Celsius to Kelvin:
T(Kelvin) = T(Celsius) + 273.15
Now, let's plug in the values into the ideal gas law equation:
P = 0.500 atm
V = 2.00 L
T = 50.0 degrees C = 50.0 + 273.15 = 323.15 K
R = 0.0821 L.atm/mol.K
PV = nRT
(0.500 atm)(2.00 L) = n(0.0821 L.atm/mol.K)(323.15 K)
1.00 atm.L = n(26.62 L.atm/mol)
n = (1.00 atm.L) / (26.62 L.atm/mol)
n ≈ 0.0376 moles
Therefore, approximately 0.0376 moles of methane occupy a volume of 2.00 L at 50.0 degrees C and 0.500 atm.