Given, pressure = P = 800 mm Hg = 1.066 X 10^5 Pa Volume = V = 55 l = 0.055 m^3 number of moles of Cl2 gas = n = [tex] \frac{weight}{\text{molecular weight}} [/tex] = [tex] \frac{100}{71} [/tex] = 1.408
Now, based on ideal gas equation, we have PV=nRT ∴ T = PV/RT where R = universal gas constant = 8.314 J /mol K ∴ T = [tex] \frac{1.066X 10^5X0.055}{1.408X8.314} [/tex] = 500.8 K
Now, we know that [tex] 0^{0}C = 273.15 K [/tex] ∴ 500.8 K = [tex] 227.65^{0}C [/tex]
