what is the density of carbon tetrachloride vapor at 0.975 atm and 125 celsius

125 C = 398 K

molar mass of CCl4 = 12 + 4*35.5 = 154 g/mol

22.4 liters of an ideal gas contains 1 mole at STP, or 0.975*(273/398) = 0.6688 moles at 0.975 atm and 398 K.

density of CCl4 = 0.6688*154 g/(22.4 l)
= 4.60 g/l

You could also calculate moles per volume using
n/V = P/RT
and multiply that by the molar mass.

Oh, carbon tetrachloride vapor at a party? Let's see, at 0.975 atm and 125 degrees Celsius, the density of carbon tetrachloride vapor is... drum roll, please... approximately 3.22 kg/m³. So, it's quite light, almost as light as a feather...well, maybe not that light, but you get the idea!

To find the density of carbon tetrachloride vapor at a specific pressure and temperature, 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 ideal gas constant, and T is the temperature.

First, we need to determine the number of moles of carbon tetrachloride gas. We can use the ideal gas law and rearrange it to solve for n:

n = PV / RT

Where:
P = 0.975 atm (pressure)
V = unknown (volume)
R = 0.08206 L∙atm/(mol∙K) (ideal gas constant)
T = 398.15 K (converted from 125 °C)

Now, we need to solve for the volume (V) in the ideal gas law equation. To do this, we rearrange the equation as:

V = (nRT) / P

Substituting the given values:

n = (0.975 atm) x (V) / (0.08206 L∙atm/(mol∙K)) x (398.15 K)

Now, let's assume the volume is 1 liter (V = 1 L):

n = (0.975 atm) x (1 L) / (0.08206 L∙atm/(mol∙K)) x (398.15 K)

Calculating this will give us the number of moles (n) of carbon tetrachloride. Then, we can find the molar mass of carbon tetrachloride using the periodic table.

Finally, we can calculate the density using the formula:

Density = (Molar mass) / (Volume)

Please note that to calculate the density accurately, it's necessary to know the molar mass of carbon tetrachloride, which is 153.82 g/mol.

Let's calculate the density assuming the volume is 1 liter.

To find the density of carbon tetrachloride vapor at 0.975 atm and 125 degrees Celsius, we can use the ideal gas law and the molar mass of carbon tetrachloride (CCl4).

Here are the steps to calculate the density:

1. Convert the temperature from Celsius to Kelvin by adding 273.15.
Temperature in Kelvin = 125 + 273.15 = 398.15 K

2. Convert the pressure from atm to Pascals (Pa) by multiplying by 101,325.
Pressure in Pa = 0.975 atm * 101,325 Pa/atm = 98,708.375 Pa

3. Calculate the molar mass of carbon tetrachloride (CCl4). The molar mass of C = 12.01 g/mol, and the molar mass of Cl = 35.45 g/mol.
Molar mass of CCl4 = (12.01 g/mol * 1) + (35.45 g/mol * 4) = 153.82 g/mol

4. Calculate the density using the ideal gas law formula: PV = nRT.
Density = (molar mass * P) / (R * T)
where P is the pressure in Pascals, R is the ideal gas constant (8.31 J/(mol·K)), T is the temperature in Kelvin, and n is the number of moles.

Density = (153.82 g/mol * 98,708.375 Pa) / (8.31 J/(mol·K) * 398.15 K)

5. Convert the density from grams to kilograms by dividing by 1000.
Density in kg/m^3 = (Density in g/m^3) / 1000

After performing the calculations, the density of carbon tetrachloride vapor at 0.975 atm and 125 degrees Celsius is the calculated value in kg/m^3.