We will assume that the gas behaves like an ideal gas, so we can apply the following equation for ideal gases:
[tex]PV=nRT[/tex]Where,
P is the pressure of the gas, in atm
V is the volume of the gas in liters, 67.153L
n is the moles of the gas, 6.7969 mol
T is the temperature of the gas in Kelvin, 668.44°C=947.59K
R is a constant, 0.08206atm.L/mol.K
Now, we clear the pressure and replace the known data:
[tex]P=\frac{nRT}{V}[/tex][tex]P=\frac{6.7969mol\times0.08206\frac{atm.L}{mol.K}\times947.59K}{67.153L}=7.8206atm[/tex]Answer: The pressure of this gas is 7.8206atm
