(Solved): Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br2(g) ...

Molecular bromine, $${\mathrm{Br}}_2$$, dissociates at elevated temperatures into bromine atoms, $$\mathrm{Br}$$. $${\mathrm{Br}}_2(g)?2\mathrm{Br}(g)$$ A $$2.570\mathrm{L}$$ flask initially contains pure molecular bromine. The temperature is then raised to $$1.600\times 10^3\mathrm{K}$$. The total pressure of this equilibrium mixture at this elevated temperature is $$1.000\mathrm{atm}$$. A spectroscopic analysis of this mixture showed that it contained $$1.197\mathrm{g}$$ of $$\mathrm{Br}$$ atoms. a. What are the total moles of gas in the container? $$\mathrm{mol}$$ b. What is the partial pressure of $$\mathrm{Br}$$ ? $$\mathrm{atm}$$ c. What is $$K_p$$ for the dissociation of molecular bromine to bromine atoms? $$K_p=$$ 3 item attempts remaining