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]