The Determination of a Rate Equation

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The Determination of a Rate Equation

Aim

---

The purpose of this experiment is to develop a method to determine the

rate equation for the reaction between Magnesium ribbon and 2.0mol dm

Hydrochloric acid, HCl.

Hypothesis and Theory

---------------------

When I react the magnesium ribbon with hydrochloric acid they will

undergo the reaction according to the equation below:

Mg(s) + 2HCl(aq) à MgCl (aq) + H (g)

For a reaction to be successful the molecules must collide with

sufficient kinetic energy in order to surmount the energy barrier,

also known as the activation energy. When there is an increased

concentration of reactants then there is a greater chance of these

successful collisions occurring therefore speeding up the reaction (As

How far, How fast?).

According to the collision theory, I should expect that as I increase

the concentration of hydrochloric acid then the reaction rate would

also increase because a higher frequency of collisions will increase

the rate of reaction. Therefore increasing the time taken for the

magnesium to dissolve.

When the magnesium ribbon is added to hydrochloric acid effervescence

is expected as they begin to react providing me with a reliable method

of measuring the reaction rate, hence the time taken for the magnesium

wire to completely dissolve.

Accuracy measures and Varying Factors

-------------------------------------

Ø The length of the magnesium ribbon will have to be kept to 0.03g on

each trial.

Ø The temperature of the hydrochloric acid should remain constant

throughout the trials and each concentration temperature should be

checked with a thermometer of 0.5 accuracy. Varying temperatures

increase kinetic energy therefore increasing the vibrations and then

the frequency of successful collisions. Any variations in temperature

may skew results as I am investigating the effect of hydrochloric acid

concentration on the rate and not temperature.

Ø Start the clock as soon as the magnesium ribbon is added to the

hydrochloric acid.

Ø Measure solutions as accurately as possible by making sure the

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