The gase in a mixture have the following partial pressures at the same volume and temperature, 1013000Pa nitrogen, 700mm argon, 1.20atm helium, 790 torr oxygen, and 0.50 atm of carbon dioxide. What is the total pressure of tyhe mixture in atm?
You add them. You will have to convert units to the same units.
760torr= 1atm= 101.3kPa= 760mmHg
To find the total pressure of the mixture, we need to add up the partial pressures of all the gases. However, we first need to convert all the partial pressures to the same units.
Given:
Nitrogen partial pressure = 1013000 Pa
Argon partial pressure = 700 mm
Helium partial pressure = 1.20 atm
Oxygen partial pressure = 790 torr
Carbon dioxide partial pressure = 0.50 atm
To convert the units to the same base unit, we will use the following conversions:
1 atm = 760 mmHg (torr)
1 atm = 101.3 kPa
1 atm = 101325 Pa
Converting the given data to the same units:
Nitrogen partial pressure = 1013000 Pa
Argon partial pressure = 700 mmHg (torr) (no conversion needed as it is already in the desired unit)
Helium partial pressure = 1.20 atm
Oxygen partial pressure = 790 torr
Carbon dioxide partial pressure = 0.50 atm
Now let's convert the oxygen and carbon dioxide partial pressures to atm and mmHg (torr):
Oxygen partial pressure = 790 torr = 790 torr * (1 atm / 760 torr) = approximately 1.0395 atm
Carbon dioxide partial pressure = 0.50 atm
Now we have all the partial pressures in the same units (atm). We can proceed to add them up:
Total pressure = Nitrogen partial pressure + Argon partial pressure + Helium partial pressure + Oxygen partial pressure + Carbon dioxide partial pressure
Total pressure = 1013000 Pa + 700 mmHg + 1.20 atm + 1.0395 atm + 0.50 atm
Now, we can convert back to atm if needed:
Total pressure = (1013000 Pa / 101325 Pa/atm) + (700 mmHg / 760 mmHg/atm) + 1.20 atm + 1.0395 atm + 0.50 atm
Simplifying the expression by performing the conversions and additions, we get:
Total pressure = 9.993 atm
Therefore, the total pressure of the gas mixture is approximately 9.993 atm.