a vessel has 6 g oxygen at a pressure P & temp 400 K . a small hole is made in it so that oxygen leaks out . how much oxygen leaks out if the pressure is P/2 & temperature 300 K ?
1. 5g
2. 4g
3. 2g
4. 3g
Use PV = nRT. To make things easier, I would assign P = 1 for initial P and 0.5 for the second run. Calculate V.
Then use PV = nRT with new conditions but solve for n and convert to grams. Subtract from the 6 g initially. Post your work if you get stuck.
Dr Bob222 can u post the answer ?
To determine how much oxygen leaks out of the vessel, we can use the ideal gas law equation, which is given as:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles of gas
R = Ideal gas constant
T = Temperature
Now, since the temperature and pressure have changed, we need to use the equation in two different scenarios and compare the results:
1. For the initial conditions (P, T, and n):
P1 = P
T1 = 400 K
n1 = mass/Molar mass
2. For the final conditions (P/2, T, and n):
P2 = P/2
T2 = 300 K
n2 = mass/Molar mass
To calculate the number of moles in each scenario, first, we need to find the molar mass of oxygen, which is 32 g/mol (approximately).
Now we can use the ideal gas law equation to solve for the mass of oxygen (m) in each scenario:
1. For the initial conditions:
PV = nRT
P1V = (mass/Molar mass) * R * T1
mass1 = (P1V * Molar mass) / (R * T1)
2. For the final conditions:
P2V = (mass/Molar mass) * R * T2
mass2 = (P2V * Molar mass) / (R * T2)
To find the amount of oxygen that leaks out, we calculate the difference in mass:
leaked_out = mass1 - mass2
Finally, we substitute the known values into the equations and calculate the answer.