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 u2234 T = PV/RT where R = universal gas constant = 8.314 J /mol K u2234 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] u2234 500.8 K =[tex] 227.65^{0}C [/tex]

## Answers ( 1 )

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

u2234 T = PV/RT

where R = universal gas constant = 8.314 J /mol K

u2234 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]

u2234 500.8 K =[tex] 227.65^{0}C [/tex]