Iodine monochloride, ICl, is a brown liquid. It reacts with chlorine gas to form iodine trichloride, ICl3\mathrm{ICl_{3}}ICl3, a yellow solid.
ICl(l)+Cl2(g)⇌ICl3(s) \mathrm{ICl(l) + Cl_{2}(g) \rightleftharpoons ICl_{3}(s)} ICl(l)+Cl2(g)⇌ICl3(s)A mixture of the brown liquid and the yellow solid is at equilibrium in a closed tube containing chlorine gas. Some of the chlorine gas is removed from the tube.
What is observed?
More brown liquid forms, because the position moves to the left.
More yellow solid forms, because the position moves to the right.
No change is seen, because removing a reactant has no effect.
More yellow solid forms, because the chlorine left reacts faster.
47 exam-style questions on OCR GCSE Chemistry 5.3 Equilibria, covering 5.3.1 Reversible reactions and dynamic equilibrium and 5.3.2 Changing the position of equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.