Calculate the density of sulfur hexafluoride gas at 703 torr and 23°C.
density is mass/volume so how do i get those from what i am given?
also
) Calculate the molar mass of a vapor that has a density of 6.735 g/L at 11°C and 743 torr.
Molar mass SF6 = 146.06 g/mol
p = 723 / 760 = 0.951 atm
T = 31 + 273 = 304 K
d = M p / RT = 146.06 x 0.951 / 0.0821 x 304 = 5.57 g/L
M = d x RT/ p
T = 14 + 273 = 287 K
p = 825 / 760 = 1.09 atm
M = 7.535 x 0.0821 x 287 / 1.09 = 162.89 g/mol
Hope this helps :)
thanks!!!
Well, to calculate the density of sulfur hexafluoride gas at 703 torr and 23°C, you need to know the molar mass of sulfur hexafluoride (SF6). From there, you can use the ideal gas law to find the density.
As for obtaining the mass and volume, you can use the following formulas:
Mass = Density × Volume
Volume = (RT)/P
Where:
R is the ideal gas constant (0.0821 L·atm/mol·K),
T is the temperature in Kelvin (23°C + 273.15 = 296.15 K), and
P is the pressure in atm (703 torr / 760 torr/atm = 0.9237 atm).
However, as a Clown Bot, I must confess that I don't know the molar mass of sulfur hexafluoride off the top of my head, nor do I have the capacity to perform calculations. But hey, at least I can entertain you with some silly jokes while you work on the calculations!
To calculate the density of a gas, we need to use the ideal gas law:
PV = nRT
where:
- P is the pressure in atm,
- V is the volume in liters,
- n is the number of moles of gas,
- R is the ideal gas constant (0.0821 L.atm/mol.K), and
- T is the temperature in Kelvin.
Let's convert the given values:
- Pressure = 703 torr = 703/760 atm = 0.924 atm
- Temperature = 23°C = 23 + 273.15 = 296.15 K
Now, we need to rearrange the ideal gas law to solve for density. The density (d) is given by:
d = (molar mass) * (P / (R * T))
To find the molar mass, we need to rearrange the equation:
molar mass = (density * R * T) / P
Now let's calculate the density of sulfur hexafluoride (SF6) gas at 703 torr and 23°C:
Using the given values:
Pressure (P) = 0.924 atm
Temperature (T) = 296.15 K
Note: The molar mass of SF6 is 146.06 g/mol.
First, we find the molar mass:
molar mass = (density * R * T) / P
molar mass = (density * 0.0821 L.atm/mol.K * 296.15 K) / 0.924 atm
Now we can plug in the given density of 6.735 g/L and solve for molar mass:
molar mass = (6.735 g/L * 0.0821 L.atm/mol.K * 296.15 K) / 0.924 atm
molar mass = 246.134 g/mol
So, the molar mass of the vapor is 246.134 g/mol.
To calculate the density of sulfur hexafluoride gas at 703 torr and 23°C, we first need to find the mass and volume.
1. Mass: To determine the mass, we need to know the molar mass of sulfur hexafluoride (SF6). Sulfur (S) has a molar mass of 32.06 g/mol, and each fluorine (F) atom has a molar mass of 18.998 g/mol. Since there are six fluorine atoms, the total molar mass of SF6 is:
Molar mass of sulfur hexafluoride (SF6) = (1 * molar mass of sulfur) + (6 * molar mass of fluorine)
= (1 * 32.06 g/mol) + (6 * 18.998 g/mol)
= 32.06 g/mol + 113.99 g/mol
= 146.05 g/mol
2. Volume: To determine the volume, we can make use of the ideal gas equation:
PV = nRT
Where:
P = pressure (703 torr)
V = volume
n = number of moles (which we will calculate using the ideal gas equation)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (23°C = 273 + 23 = 296 K)
Rearranging the equation to solve for volume:
V = (nRT) / P
Now, let's calculate the number of moles using the ideal gas equation:
n = PV / RT
= (703 torr * 1 atm/760 torr) * V / (0.0821 L·atm/mol·K * 296 K)
= (703/760) * V / (0.0821 * 296) mol
Substituting the known values, the expression simplifies to:
n = 0.908 * V
Now, we can substitute the value of n into the equation V = (nRT) / P:
V = (0.908 * V * 0.0821 * 296) / 703 L/mol
703 = 0.908 * 0.0821 * 296
V = (703) / (0.908 * 0.0821 * 296) L
Now that you have the volume, you can proceed to calculate the density:
Density = mass / volume
Density = (molar mass * n) / V
= (146.05 g/mol * 0.908 * V) / V
= 132.65 g/L
Therefore, the density of sulfur hexafluoride gas at 703 torr and 23°C is 132.65 g/L.
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Now, let's move on to calculating the molar mass of the vapor with a density of 6.735 g/L at 11°C and 743 torr.
To determine the molar mass of the vapor, we can use the ideal gas equation.
Given:
Density = 6.735 g/L
Temperature (T) = 11°C = 11 + 273 = 284 K
Pressure (P) = 743 torr
Using the ideal gas equation, PV = nRT, we can solve for the number of moles (n):
n = PV / RT
= (743 torr * 1 atm/760 torr) * (1 L) / (0.0821 L·atm/mol·K * 284 K)
= (743/760) / (0.0821 * 284) mol
≈ 0.387 mol
Now, we can calculate the molar mass:
Molar mass = mass / moles
Since we are given the density in g/L, we can determine the mass using the density and volume:
Mass = Density * Volume
= 6.735 g/L * 1 L
= 6.735 g
Finally, we can calculate the molar mass:
Molar mass = mass / moles
= 6.735 g / 0.387 mol
≈ 17.39 g/mol
Therefore, the molar mass of the vapor is approximately 17.39 g/mol.