A gas mixture containing 0.400 mol He, 0.184 mol CH4 and 0.0374 mol Ne was placed in a 3.00-L flask at 301 K. What is the PRESSURE (atm) in the flask?
sad no one helped me
Use PV = nRT
P = ?
V = 3 L
n = sum of mols.
R is gas constant
T must be in kelvin.
518
To find the pressure in the flask, we can use the ideal gas law equation:
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)
We have:
n₁ = 0.400 mol He
n₂ = 0.184 mol CH₄
n₃ = 0.0374 mol Ne
Adding up the number of moles, we get:
ntotal = n₁ + n₂ + n₃
Now, let's solve for the pressure (P):
P = (ntotal * R * T) / V
Substituting the given values:
V = 3.00 L
T = 301 K
Calculating the total number of moles:
ntotal = 0.400 + 0.184 + 0.0374
Now we can put the values into the equation and solve for P:
P = (ntotal * R * T) / V