How many moles of helium gas (He) would be required to fill a 22 L container at a temperature of 35oC and a pressure of 3.1 atm?
Use PV = nRT and solve for n = PV/RT
P = 3.1 atm
V = 22 L
R = 0.08205 L*atm/mol*K
T = 35 C + 273 = ? K.
Substitute these values and solve for n.
2.69
To calculate the number of moles of helium gas (He) required to fill a 22 L container at a temperature of 35°C and a pressure of 3.1 atm, you can use the ideal gas law. The ideal gas law equation is given as:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature (in Kelvin)
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15:
T = 35°C + 273.15 = 308.15 K
Now, we can rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (3.1 atm) * (22 L) / ((0.0821 L·atm/mol·K) * (308.15 K))
Calculating this expression will give us the number of moles of helium gas required to fill the 22 L container at the given conditions.
To calculate the number of moles of helium gas required to fill a 22 L container at a given temperature and pressure, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles of gas
R = Gas constant (0.0821 L·atm/mol·K)
T = Temperature (in Kelvin)
First, we need to convert the temperature from Celsius to Kelvin:
T(Kelvin) = T(Celsius) + 273.15
T(Kelvin) = 35 + 273.15 = 308.15 K
Now, we can rearrange the equation to solve for the number of moles of helium gas (n):
n = PV / RT
n = (3.1 atm)(22 L) / (0.0821 L·atm/mol·K)(308.15 K)
n = 1.54 moles
Therefore, approximately 1.54 moles of helium gas would be required to fill a 22 L container at a temperature of 35oC and a pressure of 3.1 atm.