Answer:
3.16g/L
Explanation:
We'll begin by obtaining an equation for the density. This is illustrated below:
From the ideal gas equation:
PV = nRT (1)
But n = Mass(m) /Molar Mass (M)
n = m/M
Substituting the value of n into equation 1, we have:
PV = nRT
PV = mRT/M
Now, divide both side by P
V = mRT/MP
Next, divide both by m
V/m = RT/MP
Next, invert the above equation
m/V = PM/RT. (2)
Recall:
Density (D) = Mass (m) /Volume (V)
D = m/V
Now, replace m/V in equation 2 by D, we have:
m/V = PM/RT
D = PM/RT
Data obtained from from the question include:
P (pressure) = stp = 1atm
T (temperature) = stp = 273K
R (gas constant) = 0.0821atm.L/Kmol
M (molar mass of Cl2) = 2 x 35.45 = 70.9g/mol
D (Density) =?
Now, applying the derived formula D = PM/RT, the density of chlorine gas (Cl2) can be obtained as follow:
D = PM/RT
D = (1 x 70.9)/(0.0821 x 273)
D = 3.16g/L
Therefore, the density of the chlorine gas is 3.16g/L