Final answer:
The virial pressure of 0.654 moles of F6S gas at 350 K in a 1000 cm3 container, given B=-190 cm³/mol, is 16.72 atm. The negative virial coefficient indicates attractive forces are present. Increase in temperature would likely make the virial coefficient less negative.
Step-by-step explanation:
The virial equation of state for a non-ideal gas is given by:
PV = nRT(1 + B'P + C'P² + ...)
However, to find the virial pressure with the given second virial coefficient B, the equation simplifies to:
P = (nRT/V) / (1 - nB/V)
Substituting the values:
Now we calculate the pressure:
P = (0.654 moles * 0.0821 L·atm/(K·mol) * 350 K) / (1 L - 0.654 moles * -0.190 L/mol)
P = (18.80655 atm·K·mol / L·K) / (1 L + 0.12426 L)
P = 18.80655 atm / 1.12426
P = 16.72 atm (to two significant figures)
The negative sign of the virial coefficient indicates that attractive forces are present under these conditions. If the temperature of this gas were to increase, the virial coefficient would likely become less negative, signifying a reduction in the magnitude of attractive forces or an increase in repulsive forces as the gas particles move faster and have higher energy.