How many air molecules are in a 12.0*12.0*10.0 ft room? Assume atmospheric pressure of 1.00 atm, a room temperature of 20.0 degree Celsius , and ideal behavior.

Volume conversion:There are 28.2 liters in one cubic foot.

Oh, calculating the number of air molecules in a room? That's a breath-taking question! Let me entertain you with a clown-inspired calculation.

First, let's convert the room volume into liters. So, 12.0 * 12.0 * 10.0 ft = 1,728 cubic feet. Multiply that by 28.2 liters/cubic foot, and you get a grand total of 48,641.6 liters.

Now, let's use the Ideal Gas Law to find the number of moles of air in the room. We'll need the formula: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

Since we know the pressure is 1.00 atm, the volume is 48,641.6 liters, and the temperature is 20.0 degrees Celsius (or 293.15 Kelvin), we can plug those numbers in.

1.00 atm * 48,641.6 L = n * 0.0821 L·atm/(mol·K) * 293.15 K

Let's simplify: 48,641.6 = n * 24 (approx.)

Finally, divide both sides by 24, and you'll find that the number of moles of air in the room is approximately 2,027.6 moles.

But, remember that each mole contains Avogadro's number of air molecules, which is about 6.022 × 10^23. So, multiply our number of moles by that, and you're left with a final answer of approximately 1.22 × 10^27 air molecules in that room!

That's an air-raising number, isn't it? I hope my calculations added a hilarious touch to your day!

To calculate the number of air molecules in a room, we need to use the ideal gas equation, which is given by:

PV = nRT

Where:
P = pressure (atm)
V = volume (liters)
n = number of moles of gas
R = ideal gas constant
T = temperature (Kelvin)

First, let's convert the room volume from cubic feet to liters.

Given:
Room volume = 12.0 ft * 12.0 ft * 10.0 ft
Volume conversion: 1 cubic foot = 28.2 liters

Room volume in liters = (12.0 ft * 12.0 ft * 10.0 ft) * (28.2 liters/1 cubic foot)

Next, we need to convert the room temperature from Celsius to Kelvin.

Given:
Room temperature = 20.0 degrees Celsius

Temperature in Kelvin = 20.0 degrees Celsius + 273.15

Now, we can plug the values into the ideal gas equation.

PV = nRT

We know:
P = 1.00 atm (atmospheric pressure)
V = room volume in liters (calculated above)
R = 0.0821 L·atm/(K·mol) (ideal gas constant)
T = room temperature in Kelvin (converted above)

Solving for n, we can calculate the number of moles of air in the room.

n = (P * V) / (R * T)

Substituting the given values, we can find the number of moles of air in the room.

Finally, we can multiply the number of moles of air by Avogadro's number (6.022 x 10^23) to get the number of air molecules.

So, to get the answer to the question, you would need to follow these steps:

1. Convert the room volume from cubic feet to liters using the given conversion factor.
2. Convert the room temperature from Celsius to Kelvin.
3. Plug the values of pressure, volume, ideal gas constant, and temperature into the ideal gas equation (PV = nRT) to calculate the number of moles of air.
4. Multiply the number of moles of air by Avogadro's number to get the number of air molecules in the room.

You need to

1. calculate the volume of the room

2. Convert the volume to litres

3. Use PV=nRT to calculate the number of moles of gas (n). Remember to use the correct value for R and convert temperature to K.

3. multiply the number of moles (n) by Avogadros' number (6.023 x 10^23) to get the number of air molecules.

6.97*10^21

8.89*10^26 is the correct answer