Carbonyl bromide, COBr2, decomposes into carbon monoxide and bromine according to the following balanced equation:
COBr2(g) ⇌ CO(g) + Br2(g) ∆H > 0
Initially COBr2(g) is sealed in a 2 dm3 container and heated to 73 °C. The reaction is
allowed to reach equilibrium at this temperature. The equilibrium constant for the
reaction at this temperature is 0,19.
6.1 Define chemical equilibrium. (2)
At equilibrium it is found that 1,12 g CO(g) is present in the container.
6.2 Calculate the:
6.2.1 Equilibrium concentration of the COBr2(g) (7)
6.2.2 Percentage of COBr2(g) that decomposed at 73 °C (4)
6.3 Which ONE of the following CORRECTLY describes the Kc value when equilibrium is reached at a lower temperature?
6.4 The pressure of the system is now decreased by increasing the volume of the container at 73 °C and the system is allowed to reach equilibrium.
How will the number of moles of COBr2(g) be affected? Choose from INCREASES, DECREASES or REMAINS THE SAME. Explain the answer. (3)
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