A fire extinguisher filled with carbon dioxide has a mass of 3500g. After releasing all of the

CO2, the mass of the extinguisher is 2735g. What was the pressure reading on the gauge
before any CO2 was released, if the volume of the extinguisher is 4.25 L and it is stored
at a temperature of 25 oC?

3500 g = mass gas + container

-2735 g = mass container
-----------
765 g = mass CO2 gas

mols CO2 = grams/molar mass = n
Then use PV = nRT to dtermne P

To solve this problem, you can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = moles of gas
R = ideal gas constant
T = temperature in Kelvin

First, convert the temperature from Celsius to Kelvin:
T = 25 + 273.15 = 298.15 K

Now, let's calculate the initial number of moles by using the masses given. We know that the molar mass of carbon dioxide (CO2) is 44 g/mol.

Initial mass of the extinguisher = 3500 g
Final mass of the extinguisher = 2735 g

Mass of CO2 released = Initial mass - Final mass
Mass of CO2 released = 3500 g - 2735 g = 765 g

Convert the mass of CO2 released to moles:
Moles of CO2 = Mass of CO2 released / Molar mass of CO2
Moles of CO2 = 765 g / 44 g/mol ≈ 17.386 moles

Since there is no change in the volume, we can assume that it is constant at 4.25 L.

Now, rearrange the ideal gas law equation to solve for pressure:
P = nRT / V

Substitute the known values into the equation:
P = (17.386 moles) * (0.0821 L·atm/K·mol) * (298.15 K) / (4.25 L)

Calculating the pressure:
P ≈ 80.62 atm

Therefore, the pressure reading on the gauge before any CO2 was released was approximately 80.62 atm.

To find the pressure reading on the gauge before any CO2 was released, we can 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 in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin. We can do this by adding 273.15 to the Celsius temperature. So, 25°C + 273.15 = 298.15 K.

Next, we need to calculate the number of moles of carbon dioxide (CO2) in the fire extinguisher. We can use the molar mass of CO2, which is 44.01 g/mol. To find the moles, we divide the mass of the CO2 by the molar mass: 3500 g / 44.01 g/mol = 79.51 mol.

Now, we can rearrange the ideal gas law equation to solve for the pressure (P): P = (nRT) / V. Plugging in the values we have: P = (79.51 mol * 0.0821 atm/mol*K * 298.15 K) / 4.25 L.

Calculating this gives us a pressure of: P = 61.09 atm.

Therefore, the pressure reading on the gauge before any CO2 was released was 61.09 atm.