A 150.0 mL flask contains 740. g of N2 at 0°C.
What is the pressure in atm.
What is the pressure in torr?
What is the pressure in psi?
n = grams/molar mass
Then PV = nRT
R in 0.08206 L.atm/mol.K gives P in atm
atm x 760 = p in torr
1 atm = 14.7 psi
To determine the pressure in atm, torr, and psi, we need to use the ideal gas law equation, which is:
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 given values into the appropriate units. We know that the volume is 150.0 mL, so we need to convert it to liters by dividing by 1000:
V = 150.0 mL / 1000 = 0.150 L
The mass of N2 is given as 740. g. To determine the number of moles, we need to use the molar mass of N2, which is 28.02 g/mol:
n = 740. g / 28.02 g/mol = 26.394 mol
The temperature is given as 0°C. However, we need to convert it to Kelvin by adding 273.15:
T = 0°C + 273.15 = 273.15 K
Now we can plug the values into the ideal gas law equation to calculate the pressure:
P = nRT / V
P = (26.394 mol)(0.0821 L•atm/mol•K)(273.15 K) / 0.150 L
P = 35.6481 atm
To convert this pressure to torr, we can use the conversion factor:
1 atm = 760 torr
Therefore, the pressure in torr would be:
Pressure in torr = (35.6481 atm)(760 torr) = 27,105.576 torr
To convert the pressure to psi, we need to use the conversion factor:
1 atm = 14.696 psi
Therefore, the pressure in psi would be:
Pressure in psi = (35.6481 atm)(14.696 psi) = 524.15 psi
So, the pressure in atm is 35.6481 atm, the pressure in torr is 27,105.576 torr, and the pressure in psi is 524.15 psi.