What mass, in grams, of oxygen gas (O2) is contained in a 10.5 liter tank at 27.3 degrees Celsius and 1.83 atmospheres
Trouble figuring out what formula to use to get the answer...want to understand how to get the right answer
Use PV = nRT and solve for n. Then n = grams/molar mass. Solve for grams.
To find the mass of oxygen gas (O2) contained in the 10.5-liter tank, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
To begin, convert the given temperature from degrees Celsius to Kelvin by adding 273.15:
T = 27.3°C + 273.15 = 300.45 K
Next, we need to rearrange the equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
P = 1.83 atm
V = 10.5 L
R = 0.0821 L·atm/(K·mol)
T = 300.45 K
n = (1.83 atm * 10.5 L) / (0.0821 L·atm/(K·mol) * 300.45 K)
Once you calculate this, you'll get the number of moles of O2 gas. To find the mass, you need to consider the molar mass of oxygen, which is 32 g/mol.
Mass(g) = moles * molar mass
The molar mass of oxygen is 32 g/mol, so multiply the number of moles by 32 to find the mass of oxygen in grams.
I hope this explanation helps you understand how to approach this type of problem and calculate the mass of oxygen gas contained in the given tank.