If the pressure exerted by ozone, O3, in the stratosphere is 3.0 x 10^-3 atm and the temperature is 250K, how many ozone molecules are in a liter?

Please help me.

Why did the ozone molecule go to the party alone? Because it couldn't find any stable partners to bond with! But don't worry, I'm here to help you find the number of ozone molecules in a liter.

First, let's use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Since we want to find the number of ozone molecules in a liter, we can convert the pressure from atmospheres to Pascals (Pa), and the volume from liters to cubic meters (m³). The number of molecules, n, can then be calculated using Avogadro's number.

Let's plug in the values:

P = 3.0 x 10^-3 atm * (101,325 Pa/atm) = 303.975 Pa
V = 1 L * (1 m³/1000 L) = 0.001 m³
T = 250 K
R = 8.314 J/(mol K)

Now we can rearrange the equation to solve for n:

n = (PV) / (RT)
n = (303.975 Pa * 0.001 m³) / (8.314 J/(mol K) * 250 K)

Calculating this gives us:

n ≈ 0.146 moles

Now, we know that 1 mole of any substance contains 6.022 x 10^23 molecules according to Avogadro's number. Therefore, to find the number of ozone molecules in a liter, we multiply the number of moles by Avogadro's number:

Number of molecules = 0.146 moles * (6.022 x 10^23 molecules/mol)

Calculating this gives us:

Number of ozone molecules ≈ 8.78 x 10^22 molecules

So, there are approximately 8.78 x 10^22 ozone molecules in a liter. Keep in mind that this calculation assumes ideal gas behavior. Hope this help!

To calculate the number of ozone molecules in a liter, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)

First, we need to convert the pressure given in the problem to atm:

3.0 x 10^-3 atm

Next, we'll convert the temperature from Celsius to Kelvin:

T = 250K

Now, we can rearrange the ideal gas law equation to solve for the number of moles:

n = PV / RT

Substituting the given values into the equation, we get:

n = (3.0 x 10^-3 atm) * (1L) / ((0.0821 L·atm/mol·K) * (250K))

Simplifying further:

n = 0.000036 mol

Since there are 6.02 x 10^23 molecules in 1 mole, we can calculate the number of ozone molecules in a liter by multiplying the number of moles by Avogadro's number:

Number of ozone molecules = (0.000036 mol) * (6.02 x 10^23 molecules/mol)

Calculating further:

Number of ozone molecules = 2.17 x 10^19 ozone molecules

Therefore, there are approximately 2.17 x 10^19 ozone molecules in a liter.

To determine the number of ozone molecules in a liter, we can use the ideal gas equation, which relates the number of molecules (n) to the pressure (P), volume (V), and temperature (T) of a gas.

The ideal gas equation is given by:

PV = nRT

Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of molecules
R = Gas constant (0.0821 L.atm/mol.K)
T = Temperature (in Kelvin)

Rearranging the equation to solve for n:

n = (PV) / (RT)

Given:
Pressure (P) = 3.0 x 10^-3 atm
Volume (V) = 1 liter
Temperature (T) = 250 K

Plugging in the values:

n = (3.0 x 10^-3 atm * 1 liter) / (0.0821 L.atm/mol.K * 250 K)

Simplifying the equation:

n = (3.0 x 10^-3) / (0.0821 * 250)

Using a calculator, we can calculate the value of n:

n ≈ 0.000145 mol

To convert the moles to molecules, we can use Avogadro's number, which states that there are 6.022 x 10^23 molecules in one mole.

So, the number of ozone molecules in a liter would be:

Number of molecules = n * (6.022 x 10^23)

Plugging in the value of n:

Number of molecules ≈ 0.000145 mol * (6.022 x 10^23)

Using a calculator, we can calculate the value of the number of molecules:

Number of molecules ≈ 8.7289 x 10^19 molecules

Therefore, there are approximately 8.7289 x 10^19 ozone molecules in a liter at the given pressure and temperature.

P V = n R T

P in atm
V in liters
T in deg K

R = 0.082 L atm K mol^-1
from
http://www.cpp.edu/~lllee/gasconstant.pdf

3.0*10^-3 * 1 = n (.082)(250)
n = do the calculation for n, the number of mols
then
multiply by Avagadro's number, the number of molecules per mol