a glass jar containing .27 mol of Nitrogen with a leaky lid is heated from room temperature 22 celcis to 150 celcis. How many moles of Nitrogen remain? How many gtams?
Note the correct spelling of celsius.
I assume this is at room pressure.
I would use PV = nRT, assume 1 atm for P, substitute and solve for volume in L.
Then Use PV = nRT again, this time with volume first calculated, keep P at 1 atm and solve for n.
You can convert to g by g = mols x molar mass.
To find out how many moles of Nitrogen remain in the jar after being heated, we need to understand the concept of ideal gas law and temperature changes. The ideal gas law equation is:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
In this case, we can assume that the pressure and volume of the gas remain constant since the jar has a leaky lid. Therefore, we can simplify the equation as:
n1/T1 = n2/T2
Where:
n1 = initial number of moles
T1 = initial temperature
n2 = final number of moles (what we are trying to find)
T2 = final temperature
Given:
n1 = 0.27 mol
T1 = 22°C + 273.15 (converted to Kelvin) = 295.15 K
T2 = 150°C + 273.15 (converted to Kelvin) = 423.15 K
Now we can plug in the values into the equation:
0.27 mol / 295.15 K = n2 / 423.15 K
Cross-multiplying, we get:
n2 = (0.27 mol / 295.15 K) * 423.15 K
n2 ≈ 0.385 mol
Therefore, approximately 0.385 moles of Nitrogen remain in the jar after being heated.
To calculate the grams of Nitrogen remaining, we need to know the molar mass of Nitrogen, which is approximately 28.0134 g/mol.
So, the mass of Nitrogen remaining can be calculated as:
mass = moles * molar mass
mass = 0.385 mol * 28.0134 g/mol
mass ≈ 10.77 grams
Therefore, approximately 0.385 moles (10.77 grams) of Nitrogen remain in the jar after being heated.