Carbonyl bromide decomposes to carbon monoxide and bromine.

K_c is 0.190 at 73°C. Suppose you place 0.500 mol of COBr₂ in a 2.00-L flask and heat it to 73°C (see Study Question 17). After equilibrium has been achieved, you add an additional 2.00 mol of CO.
(a) How is the equilibrium mixture affected by adding more CO?
(b) When equilibrium is reestablished, what are the new equilibrium concentrations of COBr₂, CO, and Br₂?
(c) How has the addition of CO affected the percentage of COBr₂ that decomposed?

Data given in Question 17

Carbonyl bromide decomposes to carbon monoxide and bromine.

K_c is 0.190 at 73°C. If you place 0.0500 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 decomposed at this temperature?

Transcribed Image Text:

COBr₂(g) → CO(g) + Br₂(g)