The density of a sample of F2(g) is 1.559 g/L. If the gas is held at 755 torr, calculate the temperature.
how would i calculate the volume to use
I wouldn't worry about the volume.
p*molar mass = density*RT
You know P, molar mass, density,and R.Solve for T (in kelvin).
To calculate the volume to use in this problem, you need to use the ideal gas law equation, which is:
PV = nRT
where:
P is the pressure of the gas in atmospheres (1 atm = 760 torr),
V is the volume of the gas 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 of the gas in Kelvin.
Since the problem gives you the pressure (755 torr), you can convert it to atmospheres by dividing it by 760:
755 torr / 760 torr/atm = 0.9934 atm
Next, you need to calculate the number of moles of F2 gas. The density of the gas, given as 1.559 g/L, allows you to calculate the molar mass of F2 gas. The molar mass of F2 (fluorine gas) is 38.0 g/mol. Therefore, you can find the number of moles using the following equation:
moles = mass / molar mass
In this case, the mass is equal to the density (1.559 g/L) multiplied by the volume (which is unknown) of the gas.
Now, substitute the values into the ideal gas law equation:
(0.9934 atm) * V = (moles) * (0.0821 L·atm/mol·K) * T
You can rearrange this equation to solve for V:
V = (moles * 0.0821 L·atm/mol·K * T) / 0.9934 atm
Finally, knowing the moles (calculated from the density), the pressure, and the value of the ideal gas constant, you can rearrange the equation to solve for T.