I need help setting up this problem: A 5.0 sample of O2 is in a container at STP. What volume is the container and how many molecules of O2 in the container and how many atoms of oxygen?
Step 1: Understand the problem
The problem states that there is a 5.0 sample of O2 in a container at STP (Standard Temperature and Pressure). We need to determine the volume of the container, the number of molecules of O2 in the container, and the number of atoms of oxygen.
Step 2: Recall the conditions at STP
At STP, the temperature is 273.15 Kelvin (0 degrees Celsius) and the pressure is 1 atmosphere.
Step 3: Calculate the volume of the container
To calculate the volume, we can use the ideal gas law equation, which is 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.
Since we know the pressure is 1 atmosphere and the temperature is 273.15K, we can rearrange the formula to solve for volume.
V = nRT/P
Step 4: Convert the mass of O2 to moles
We are given a 5.0 g sample of O2. To convert this to moles, we need to know the molar mass of O2.
The molar mass of O2 is approximately 32.0 g/mol (16.0 g/mol for each Oxygen atom, multiplied by 2).
moles = mass / molar mass
Step 5: Calculate the number of molecules of O2
To calculate the number of molecules of O2, we use Avogadro's number, which states that 1 mole of any substance contains 6.022 x 10^23 particles.
Number of molecules = moles x Avogadro's number
Step 6: Calculate the number of atoms of oxygen
Each O2 molecule contains 2 oxygen atoms.
Number of atoms of oxygen = number of molecules x 2
Step 7: Plug in the values and calculate
Now, we can plug in the values into the formulas and calculate the volume, the number of molecules of O2, and the number of atoms of oxygen.
V = (nRT) / P
n = (mass of O2) / (molar mass of O2)
Number of molecules = n x Avogadro's number
Number of atoms of oxygen = number of molecules x 2
Substitute the known values into the formulas and calculate the results.
To set up this problem, we need to use the ideal gas law equation, which states:
PV = nRT
Where:
P = pressure of gas
V = volume of gas
n = number of moles of gas
R = ideal gas constant
T = temperature of gas in Kelvin
We are given that the sample of O2 is at STP (Standard Temperature and Pressure). This means the temperature is 273.15 Kelvin (0 degrees Celsius) and the pressure is 1 atmosphere (atm). The molar mass of oxygen (O2) is approximately 32.00 grams per mole.
1. To find the volume of the container, we need to rearrange the ideal gas law equation:
V = (nRT) / P
Since the pressure is given as 1 atmosphere, the equation becomes:
V = (nRT) / 1
2. We need to determine the number of moles of O2 in the sample. To do this, we divide the mass of the sample (given as 5.0 grams) by the molar mass of O2:
n = mass / molar mass
n = 5.0 g / 32.00 g/mol
3. Now that we have the number of moles (n), we can substitute it into the volume equation, along with the given values for R (0.08206 L·atm/(mol·K)) and T (273.15 K):
V = ((5.0 g / 32.00 g/mol) * 0.08206 L·atm/(mol·K) * 273.15 K) / 1
Simplifying this equation will give you the volume of the container in liters.
To calculate the number of molecules of O2 and the number of atoms of oxygen in the container, we need to use Avogadro's number. Avogadro's number is defined as 6.022 x 10^23 particles per mole.
4. The number of molecules can be calculated by multiplying the number of moles (n) by Avogadro's number:
Number of molecules = n * Avogadro's number
5. Since there are 2 oxygen atoms per O2 molecule, we can calculate the number of atoms of oxygen by multiplying the number of molecules by 2:
Number of atoms of oxygen = Number of molecules * 2
By following these steps, you can set up the problem and find the volume of the container, as well as the number of molecules of O2 and the number of atoms of oxygen in the container.
Well, 5.0 grams?
PV=nRT
You are given STP conditions, so that gives pressure and temp.
n= grams/32
solve for V
how many molecules: n*avagnumber.