Temp labreport

Hypothesis: -

The rate of reaction has a positive relationship with the temperature of the Hydrochloric Acid.

Apparatus:-

1) Test tube

2) Rubber tube (a.k.a. delivery tube)

3) Measuring cylinder X2 [1-10ml, 1-100 ml]

4) Rubber Bung

5) Stopwatch

6) HCL - 150ml

7) 5x 3 cm of magnesium ribbon

8) Trough full of water

9) Beaker - 400ml

10) Water bath

11) Electric Thermometer

Method:-

• Set up the apparatus as shown below. 
• Fill the 400ml beaker with hot, room temp or cold water according to you. And use this beaker as a water bath. 
• Obtain 25ml of HCL and place it into the test tube. Then place the test tube into the 400ml of beaker 
• Record the temperature of the acid (that is inside the test tube) when it has become stable and is not rising in temperature any longer. 
• Use the other measuring cylinder and place it full of water in the water tray that it stands upside down with the rubber tube inside it leading to the test tube. 
• Place the 3cm magnesium ribbon into the test tube and at once place the bung onto the test tube 
• Start the stopwatch the same time when placing the magnesium ribbon into the test tube. 
• Then measure the amount of gas produce in 20sec
• And record the temperature of the HCL again to see the change. 
• Repeat the experiment with different temperature of HCL.

Variables:-

Dependent : Reaction rate [in the form of the volume of the gas (Hydrogen) produced in 20s]

Independent: Temperature of HCL

Constant:

• Length of magenium strip 
• Volume of HCl [25ml] 
• Concentration of HCl [0.5moles/dm3] 
• Apparatus 
• Time per reaction 
• Surroundings - pressure/place of exp/ surrounding temp/ etc.

Diagram:-

Result:-

Table Showing Volume Of Gas [cm3] Produced in 20 sec and Volume Of Gas

[cm3] Produced Each Sec In Different Temperature Showing Start And End Temperature [°C]

* Anomoly

Graph: -

Observation:- 

As we can see, the rise in temperature leads to a rise of gas produced. However, doubling the temperature does not exactly double the amount of Hydrogen produced. Also, in the result there is one result which is an anomaly as it does not follow the trend seen on the graph. Therefore, it was not included in our graph.

Conclusion:- 

As we can see clearly in the results above, as the temp increases the volume of gas increases this is because changes in temperature change the kinetic energy of the particles and hence the numbers of successful collisions increase, they collide with even more energy to break existing bonds and hence, react faster. As a result of this, the reaction takes less time to occur. therefore, we can conclude that the rate of reaction DOES have a positive relationship with the temperature of the solution & my hypothesis proved correct,

Evaluation: -

A few errors occurred during the experiment, which could be the reason for a few inaccuracies. An unexpected problem we faced was when the amount of Hydrogen produced in 15 seconds was so great that it passed the 10 cm3 mark as the measuring cylinder was too small. Hence, we estimated the volume to be 11.6 cm3. The timing also went wrong, slightly, as the bung was not removed exactly after 20 seconds of the reaction. Another problem we faced was reading the exact volume in the 20sec as we could have misread it. After dropping the magnesium ribbon, it also took time to put the bung tightly on the test tube; this could have let some Hydrogen gas produced to escape from the test tube. Also, a few times there were tiny air bubbles already present in the measuring cylinder in the tub of water, which may have been overlooked.