Involvement of catalysts in reactions

Demonstration

Catalysts provide an alternative route for reactions to proceed. They are involved in the progress of the reaction. This reaction involves the oxidation of potassium sodium tartrate by hydrogen peroxide using a cobalt salt as a catalyst. This is an exciting and spectacular demonstration.
 

Health & Safety and Technical notes

Read our standard health & safety guidance

Wear eye protection.

Potassium sodium tartrate (Rochelle salt), KNaC₄H₄O₆.4H₂O(s) - see CLEAPSS Hazcard.

Hydrogen peroxide solution, H₂O₂(aq), (IRRITANT) - see CLEAPSS Hazcard and CLEAPSS Recipe Book. The 20 'vol' solution is best made by diluting fresh 100 'vol' hydrogen peroxide solution (HARMFUL, wear goggles and consider wearing gloves) for this demonstration.

Cobalt(ll) chloride solution, CoCl₂(aq), (TOXIC) - see CLEAPSS Hazcard and CLEAPSS Recipe Book. Dissolve 0.2 g of cobalt(II) chloride-6-water (TOXIC, DANGEROUS FOR THE ENVIRONMENT) in 5 cm³ of distilled or deionised water.   

Procedure

a Weigh 5 g of the potassium sodium tartrate into a 250 cm³ beaker. Add 60 cm³ of distilled water and stir to dissolve the solid. 

b Add 20 cm³ of 20 volume hydrogen peroxide solution to the solution in the beaker. Note any signs of reaction.

c Put the beaker on the tripod and gauze and heat the mixture in the beaker to about 70 °C. Note any signs of reaction.

d Add 5 cm³ of cobalt(ll) chloride solution to the mixture in the beaker. Take care to avoid skin contact. Note any colour changes and gas produced.

Teaching notes

It is worthwhile trying this experiment before carrying out in class, because it is important to note the colour changes that occur when carbon dioxide gas is evolved.

This is an impressive demonstration of how a catalyst is involved in the progress of a reaction. Students can add another 10 cm³ of the hydrogen peroxide solution and if there is any potassium sodium tartrate remaining they will see a similar reaction.

The reaction is an oxidation of the tartrate ion (proper name is 2, 3-dihydroxybutandioate ion) to carbon dioxide gas and the methanoate ion. Hydrogen peroxide oxidises the tartrate ion very slowly if there is no catalyst, even at elevated temperatures.

Cobalt(ll) ions are pink. The hydrogen peroxide initially oxidises the cobalt(II), Co²⁺, to cobalt(lll), Co³⁺, which is green. The cobalt(III) bonds to the tartrate ion, allowing the oxidation to take place. The CO³⁺ is then reduced back to CO²⁺ and the pink colour returns.

The cobalt catalyst provides an alternative route for the reaction to occur. This alternative route has a lower activation energy and the reaction proceeds much more quickly.

Health & Safety checked February 2008

Weblinks

Royal Society of Chemistry (RSC) - offers information about the ‘Traffic light’ experiment which can be done as a demonstration