ENERGY CHANGES

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GCSE CHEMISTRY PAPER 1

ENERGY CHANGES

Start

4.5.2.2 Fuel cells

4.1 4.5.1.1 Energy transfer during exothermic and endothermic reactions

INDEX

4.5.1.2 Reaction profiles

4.5.1.3 The energy change of reactions (HT only)

4.5.2.1 Cells and batteries

CONSERVATION OF ENERGY

Energy is conserved in chemical reactions. The amount of energy in the universe at the end of a chemical reaction is the same as before the reaction takes place. If a reaction transfers energy to the surroundings the product molecules must have less energy than the reactants, by the amount transferred.

EXOTHERMIC REACTIONS

An exothermic reaction is one that transfers energy to the surroundings so the temperature of the surroundings increases. Exothermic reactions include combustion, many oxidation reactions and neutralisation. Everyday uses of exothermic reactions include self-heating cans and hand warmers.

ENDOTHERMIC REACTIONS

An endothermic reaction is one that takes in energy from the surroundings so the temperature of the surroundings decreases. Endothermic reactions include thermal decompositions and the reaction of citric acid and sodium hydrogencarbonate. Some sports injury packs are based on endothermic reactions.

REACTION PROFILES

WHAT IS ACTIVATION ENERGY? The minimum amount of energy that particles must have to react ---------------------------- Chemical reactions can occur only when reacting particles collide with each other and with sufficient energy.

THE ENERGY CHANGE OF REACTIONS

During a chemical reaction: • energy must be supplied to break bonds in the reactants • energy is released when bonds in the products are formed. In an exothermic reaction, the energy released from forming new bonds is greater than the energy needed to break existing bonds. In an endothermic reaction, the energy needed to break existing bonds is greater than the energy released from forming new bonds.

THE ENERGY CHANGE OF REACTIONS

The energy needed to break bonds and the energy released when bonds are formed can be calculated from bond energies. The difference between the sum of the energy needed to break bonds in the reactants and the sum of the energy released when bonds in the products are formed is the overall energy change of the reaction.

CELLS AND BATERIES

Cells contain chemicals which react to produce electricity. The voltage produced by a cell is dependent upon a number of factors including the type of electrode and electrolyte. A simple cell can be made by connecting two different metals in contact with an electrolyte. Batteries consist of two or more cells connected together in series to provide a greater voltage. In non-rechargeable cells and batteries the chemical reactions stop when one of the reactants has been used up. Alkaline batteries are non-rechargeable. Rechargeable cells and batteries can be recharged because the chemical reactions are reversed when an external electrical current is supplied

FUEL CELLS

Supplied by an external source of fuel (e.g hydrogen) and oxygen or air. the fuel is oxidised electrochemically within the fuel cell to produce a potential difference Overall reaction a hydrogen fuel cell involves the oxidation of hydrogen to produce water Hydrogen fuel cells offer a potential alternative to rechargeable cells & batteries Hydrogen-oxygen fuel cells The overall reaction in a hydrogen-oxygen fuel cell is: hydrogen + oxygen → water 2H2(g) + O2(g) → 2H2O(l) Electrode half equations - Higher At the negative electrode: 2H2 + 4OH- → 4H2O + 4e- At the positive electrode: O2 + 2H2O + 4e- → 4OH- When you add these two half equations together, you get the following overall equation: 2H2 + 4OH- + O2 + 2H2O + 4e- → 4H2O + 4e- + 4OH- The hydroxide ions, electrons and two H2O molecules will now cancel because they are on both sides, leaving the overall equation: 2H2 + O2 → 2H2O

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