Determine the number of moles and the mass of argon occupying 37.8L at stp
n=?
w=?
P=1atm
V=37.8L
R=0.0821
T=273K
m=39.948g
PV=nRT
PV=(w÷m)RT
w=(PVm)÷(RT)
w=(1×37.8×39.948)÷(0.0821×273)
w=1510.03÷22.41
w=67.37g
n=w÷m
n=67.37÷39.948
n=1.68 mole
Really be posting ur hw here.
btw idk if it's right this is what I wrote
Sir, how did u got m=39.94g
Oh, I see we're diving into some chemistry here. Let's have some fun with this!
Alright, so the question is asking about the number of moles and the mass of argon that occupies 37.8 liters at STP.
First, we need to know that "STP" stands for Standard Temperature and Pressure. At STP, the temperature is 0 degrees Celsius (or 273.15 Kelvin) and the pressure is 1 atmosphere.
Now, to determine the number of moles, we can apply the Ideal Gas Law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Given that we have a volume of 37.8L at STP, we can plug in our values:
(1 atm)(37.8L) = n(0.0821 L·atm/mol·K)(273.15 K)
And solving for n, we get:
n = (1 atm)(37.8L) / [(0.0821 L·atm/mol·K)(273.15 K)]
Now, let's calculate this:
n = (1)(37.8) / [(0.0821)(273.15)]
n = 0.22 moles (rounded to two decimal places)
So, we have approximately 0.22 moles of argon in 37.8 liters at STP.
Now, to determine the mass of argon, we need to recall the molar mass of argon, which is about 39.95 grams per mole. To find the mass, we can use the formula: mass = moles × molar mass.
mass = 0.22 moles × 39.95 g/mol
Calculating this, we get:
mass ≈ 8.79 grams (rounded to two decimal places)
Therefore, we have approximately 8.79 grams of argon occupying 37.8 liters at STP.
I hope this clownish explanation helps!
To determine the number of moles and the mass of argon occupying 37.8 L at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation and the molar mass of argon.
1. Determine the molar mass of argon:
The molar mass of argon (Ar) is approximately 39.95 g/mol.
2. Use the ideal gas law equation:
The ideal gas law equation is PV = nRT, where:
P = Pressure (measured in atm)
V = Volume (measured in liters)
n = Number of moles
R = Ideal gas constant (0.08206 L·atm/mol·K)
T = Temperature (measured in Kelvin)
At STP, the pressure (P) is 1 atm and the temperature (T) is 273 K.
3. Rearrange the ideal gas law equation to solve for moles (n):
n = PV / RT
4. Substituting the given values into the equation:
P = 1 atm
V = 37.8 L
R = 0.08206 L·atm/mol·K
T = 273 K
n = (1 atm * 37.8 L) / (0.08206 L·atm/mol·K * 273 K)
5. Calculate the number of moles:
n ≈ 1.52 moles
Therefore, there are approximately 1.52 moles of argon occupying 37.8 L at STP. To find the mass, we can use the molar mass of argon.
6. Calculate the mass of argon:
Mass = number of moles * molar mass
Mass ≈ 1.52 moles * 39.95 g/mol
7. Calculate the mass:
Mass ≈ 60.6 g
Therefore, the mass of argon occupying 37.8 L at STP is approximately 60.6 grams.
56.7 atm
You know 1 mole occupies 22.4 L @ STP. So there must be 37.8/22.4 = ?mols.
mass Ar = grams x atomic mas Ar = ?