Answer to Question #91423 in Molecular Physics | Thermodynamics for Alexis

Question

Calculate the temperature of 30 g of di-atomic chlorine ( Cl2 )
gas that occupies a volume 800 L at a pressure of 10 kPa.
(atomic mass of chlorine is 35 u ).

2903.435 C
1975.996 C
3442.844 C
905.266 C
1255.705 C

Answer 1

The classical ideal gas law states

$$pV=\frac{m}{M}RT$$

So, the temperature of di-atomic chlorine

$$T=\frac{pVM}{Rm}$$

$$=\frac{10000\:\rm{Pa}\times 0.8\:\rm{m^3}\times 70\:\rm{g/mol}}{8.3\:\rm{J/(K\times mol)\times 30\:\rm{g}}}$$

$$=2248.996\:\rm{K}=1975.996\:^{\circ}\rm{C}$$