a 3.67L flask is filled with carbon monoxide at 27 degrees C until the pressure is 1.27 atm. Calculate the total pressure after 3.42 moles of carbon dioxide has been added to the flask. (R=0.082 L-atm/K mol)
Use PV = nRT and solve for n = number of mols for 27 C and 1.27 atm.
Add 3.42 and substitute total mols into PV = nRT and solve for total P.
To calculate the total pressure after adding 3.42 moles of carbon dioxide to the flask, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = moles
R = ideal gas constant
T = temperature
First, let's calculate the initial pressure of the carbon monoxide in the flask using the ideal gas law:
P1V1 = n1RT
Given:
V1 = 3.67 L
n1 = unknown
R = 0.082 L-atm/K mol
T = 27 + 273.15 K (convert Celsius to Kelvin)
We can rearrange the equation to solve for n1:
n1 = (P1V1) / (RT)
Plugging in the values:
n1 = (1.27 atm * 3.67 L) / (0.082 L-atm/K mol * 300.15 K)
n1 ≈ 0.222 mol
Now, let's calculate the final pressure after adding 3.42 moles of carbon dioxide:
P2V2 = n2RT
Given:
V2 = 3.67 L
n2 = 3.42 mol
R = 0.082 L-atm/K mol
T = 27 + 273.15 K (convert Celsius to Kelvin)
We can rearrange the equation to solve for P2:
P2 = (n2RT) / V2
Plugging in the values:
P2 = (3.42 mol * 0.082 L-atm/K mol * 300.15 K) / 3.67 L
P2 ≈ 7.375 atm
Therefore, the total pressure after adding 3.42 moles of carbon dioxide to the flask is approximately 7.375 atm.