A scuba diver's tank contains .25 kg of oxygen compressed into a volume of 4.3 L (for oxygen, 32g = 1 mole)
Calculate the gas pressure inside the tank at 9 degrees Celsius
I posted a response below. Use moles = grams/molar mass
Then use PV = nRT for each of the others to calculate P.
To calculate the gas pressure inside the tank, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in units of force per unit area, such as pascals or atmospheres)
V = volume (in units of cubic meters or liters)
n = number of moles of gas
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in units of Kelvin)
First, we need to convert the volume from liters to cubic meters. Since 1 cubic meter is equal to 1000 liters, we have:
V = 4.3 L * (1 m^3 / 1000 L) = 0.0043 m^3
Next, we need to convert the mass of oxygen into moles using the molecular weight. Since 32g of oxygen is equal to 1 mole, we have:
mass (in kg) = 0.25 kg
molecular weight of oxygen = 32 g/mol
moles of oxygen = (0.25 kg * 1000 g/kg) / (32 g/mol) = 7.8125 mol
Now we can calculate the pressure using the ideal gas law equation. However, we need to convert the temperature from Celsius to Kelvin by adding 273.15:
T = 9°C + 273.15 = 282.15 K
Substituting the values into the ideal gas law equation, we have:
P * 0.0043 m^3 = 7.8125 mol * 8.314 J/(mol·K) * 282.15 K
P = (7.8125 mol * 8.314 J/(mol·K) * 282.15 K) / 0.0043 m^3
Calculating this expression will give us the gas pressure inside the tank at 9 degrees Celsius.