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QUESTION
Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2 (g) CO(g) + Br2 (g) Kc is 0.190 at 73C. If you place 0.500 mol of COBr2 in a 2.
Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2 (g) ↔ CO(g)+ Br2 (g)Kc is 0.190 at 73◦C. If you place 0.500 mol of COBr2 in a 2.00 L flask and heat it to 73 ◦C, what are the equilibrium concentrations of COBr2, CO, and Br2? What percentage of the original COBr2 actually decomposed at this temperature?
