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Determining the effect of the concentration of HCL over the rate of the reaction between Magnesium and Hydrochloric acid

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Introduction

Determining the effect of the concentration of HCL over the rate of the reaction between Magnesium and Hydrochloric acid Formula: Mg(s) + 2HCl (aq) � MgCl2 (aq) + H2 (g) * Aim: In this practical, we will find the relationship between the rate of reaction between Mg ribbons and Hydrochloric acid and the concentration of the acid. We want to know how this factor affects the rate of this chemical reaction. * Research Question: �How does the concentration of HCL affect the rate of reaction between Mg and HCL? * Hypothesis: Based on my knowledge on collision theory and kinetics, I can predict that the higher the concentration of the acid, more successful collisions will occur, increasing the rate of reaction. * Variables: Constant Dependent Independent Amount of HCL Time in (s) that the reaction takes to be completed * Concentration of HCL * Length of the Mg Ribbon * Apparatus Requirements: * Magnesium in ribbons * HCl (0.2mol and 1.0mol) * Chronometer * Conical Flask * Cork * Measuring Cylinders * Clamp and stand * Gas syringe * Ruler * Sandpaper NOTE: Set the apparatus in the following way: * Method: * Set the apparatus as shown above * Measure 10 ml of HCl 0.2mol in a measuring cylinder * Pour the HCl in the conical flask. ...read more.

Middle

below: * TIME: Add the value of the first concentration of the first ribbon of Mg in the first try and the same value of the second try and divide the result by two: 241+ 236 / 2 = 238.5 s Repeat the process for the two concentrations used in each one of the three lengths of Mg ribbons. * AMOUNT OF GAS: Repeat the same process as the one used in the calculation of the average of Time only that in this case, we will sue the values of the amount of Hydrogen produced in (ml): 6+4/2 =5 ml Repeat the process for the two concentrations used in each one of the three lengths of Mg ribbons. By following the two processes above, we will arrive to the following information: Table 1.3 shows the average Time that each Magnesium Ribbon took to react completely with the HCL in the two different concentrations whereas Table 1.4 shows the average amounts of Hydrogen produced from this reaction. Magnesium ribbons with their lengths in Cm Average Time in (s) HCL 0.2 mol HCL 1.0 mol 1 238.5 78 2 275.5 118.5 3 329 196.5 Magnesium ribbons with their lengths in Cm Average Amount of gas in (ml) ...read more.

Conclusion

In this case, the concentration of the acid is increased factor that, as seen in the graphs above, increases the rate of the reaction. But �why is this? The higher the concentration of the acid, the more particles will be present in a certain quantity of solute. As there is a higher amount of particles, the amount of successful collisions will also increase giving as a result, the increase of the reaction rate seen in the amount of hydrogen produced in each case. * EVALUATION OF LIMITATIONS AND ERRORS; Error Cause of error Improvement Reason for Improvement Syringe stuck The syringe could easily get stuck during the practical. Before each try, remove the syringe and clean it with a paper towel, Cleaning it with a paper towel will enable us to have a more accurate reading of the amount of gas produced. Hydrogen escape. The lapses of time in which you started the clock watch and putted the cork in the conical flask, permitted some hydrogen to escape as the reaction has already started. Ask someone to help you start the clock watch when you are going to start the test. This, in order to enable you to have more time to put the cork immediately after putting the Mg ribbon. If hydrogen escapes then the readings will be inaccurate and affect the result. ...read more.

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