How factors influence the energy change when metals are added to a metal salt solution?
Skill P : Planning Experiments
Aim:
My aim is to see what factors influence the energy change when metals are added to a metal salt solution.
Introduction:
The energy released when one metal displaces another can be used in industry, for example in the reaction of aluminium with iron oxide to weld rails together. Your task is to devise a plan to show how the temperature rise, and hence the energy cange, is affected by adding different metals to copper sulphate solution. A suitable metal woould be iron, which reacts according to the equation:
Fe(s)+CuSO4(aq)?FeSO4(aq)+Cu(s)
Prediction:
In my experiment, I can predict that when we add different metals to the Copper Sulphate liquid in forms of powder, the temperature will rise when the reaction takes place, in the polystyrene cup. The more reactive the metal the more the temperature produced, so the more energy will be given off at the end of the experiment. Our expeiment was bast around the ractivity series:
Calcium
most reactive
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
least reactive
For this experiment, I chose to use six different metals, which are in bold writing in the reactivity series, the more reactive the metals are the more heat will be produced, because the ferther away the electrons are from the nucleus, the more unreactive they are, thus energy is given off when the electrons are changed. Heats of reaction in solution are measured by allowing the heat from the reaction to be absorbed by or taken from the solution in an insulated container. My experiment is an exothermic reaction, the heat given out is absorbed by the solution, the temperature rises. Insulation reduces the amount of heat energy lost to the air which could cause my results to be not exactly wright.
Skill P : Planning Experiments
Aim:
My aim is to see what factors influence the energy change when metals are added to a metal salt solution.
Introduction:
The energy released when one metal displaces another can be used in industry, for example in the reaction of aluminium with iron oxide to weld rails together. Your task is to devise a plan to show how the temperature rise, and hence the energy cange, is affected by adding different metals to copper sulphate solution. A suitable metal woould be iron, which reacts according to the equation:
Fe(s)+CuSO4(aq)?FeSO4(aq)+Cu(s)
Prediction:
In my experiment, I can predict that when we add different metals to the Copper Sulphate liquid in forms of powder, the temperature will rise when the reaction takes place, in the polystyrene cup. The more reactive the metal the more the temperature produced, so the more energy will be given off at the end of the experiment. Our expeiment was bast around the ractivity series:
Calcium
most reactive
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
least reactive
For this experiment, I chose to use six different metals, which are in bold writing in the reactivity series, the more reactive the metals are the more heat will be produced, because the ferther away the electrons are from the nucleus, the more unreactive they are, thus energy is given off when the electrons are changed. Heats of reaction in solution are measured by allowing the heat from the reaction to be absorbed by or taken from the solution in an insulated container. My experiment is an exothermic reaction, the heat given out is absorbed by the solution, the temperature rises. Insulation reduces the amount of heat energy lost to the air which could cause my results to be not exactly wright.
