Step-by-step explanation:
When working with ideal gases we usually have to work with the formula of the ideal gas law.
P * V = n * R * T
Where P is the pressure and we usually work in atm, V is the volume in L, n is the number of moles, R is the ideal gas constant and T is the temperature in K.
R = 0.082 atm*L/(mol*K)
V = ?
We will have to convert the temperature from °C to K and the P from psi to atm.
T(K) = T(°C) + 273.15
T = (273.15 + 15) K
T = 288.15 K
1 atm = 14.696 psi
P = 16.5 psi * 1 atm/(14.696 psi)
P = 1.12 atm
We still have to find the number of moles that we have in 4.5 g sample of oxygen gas. We will use the molar mass of oxygen gas to do that.
formula of oxygen gas: O₂
atomic mass of O = 16.00 amu
molar mass of O = 16.00 g/mol
molar mass of O₂ = 2 * 16.00 g/mol
molar mass of O₂ = 32.00 g/mol
mass of O₂ = 4.5 g
n = moles of O₂ = 4.5 g/(32.00 g/mol)
n = moles of O₂ = 0.14 moles
Finally we can replace all the values that we got into the formula and solve it for the volume to get the answer to our problem.
P * V = n * R * T
V = n * R * T/P
V = 0.14 moles * 0.082 atm*L/(mol*K) * 288.15 K/(1.12 atm)
V = 2.95 L
Answer: The volume of the gas is 2.95 L.