Temperature Vs Rate of Reaction

Materials

80ml H₂S₂0₄  0.25 mol solution

80 ml HCl 1 mol solution

Calorimeter (with plastic containers)

Beakers (500ml and 250ml)

Test tubes

Graduated cylinders

Eyedroppers

Stopwatch

6x Thermometres

Ice

Procedure

Because I started my experiement with 1 mol solution of H₂S₂0₄ I had to dilute it down to 0.25 mol

Prior to the experiment, half an hour before starting turn on the calorimeter

1. Measure 6ml of HCl and place it in a test tube
2. Using a different graduated cylinder measure 6 ml of H₂S₂0₄ and place it in a separate labeled test tube
3. Get the 500ml Beaker and fill it water at  6 degrees Celsius ( If tap water isn’t cold enough add ice)
4. place the test tubes in the cold water and let sit, place a thermometer in each test tube
5. When the test tubes and water are all at 6 degrees take 2ml of HCl and place it in the calorimeters container
6. Take 2ml of H₂S₂0₄ and pour it in with the 2ml of HCl, as soon as you start pouring start the stopwatch
7. When the opacity of the substance is 0 stop the stopwatch and record the data
8. repeat last two steps for the next two trials
9. Repeat steps  1-8 for the water at different temperatures (16 degrees, 26, degrees, 36 degrees and 46 degrees)

Datatable

Conclusion and Evaluation

The data shows that there is a connection between the rate of reaction and the temperature of the reactants. And this makes sense because if the particles are hotter, they have more energy, and therefore when reacting with other particles they have greater chances of overcoming the activation energy. Some things that could be improved for this lab is that the temperatures could have been from a wider scale. Also an important thing to note is that because the eyedropper was not long enough to use to insert the substances into the calorimeter, that the solution reacted differently when poured than when squirted together. Perhaps with the eyedropper the values would be more accurate.  Thirdly if we had a larger calorimeter we could use greater amounts of reactants, meaning that reactions would take longer and the discrepancies between the reaction rates would be greater.