# Kinetics in

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timer Asked: Mar 27th, 2017
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School: Purdue University

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Chemical Kinetics
−𝐸𝑎

Equations: 𝑘 = 𝐴𝑒 𝑅𝑇

Laboratory procedure
1. Measure 50 cm3 of 1M hydrochloric acid and Pour into 100 cm3 conical flask.
2. Set up the apparatus as shown below:

3. Fill the other measuring cylinder with water.
4. Add a 3 cm strip of magnesium ribbon to the flask.
5. Note the volume of hydrogen gas given off for every 15 seconds
6. Time until no any gas is given out..

The main goal/purpose of the experiment is (what are you trying to discover in this
lab):

The main goal or purpose of the experiment is to determine the rate law for the reaction of
magnesium metal with hydrochloric acid.

The overall equation is: Mg+2HCl⟶MgCl2+H2

HCl dissociates in H2O, and forms: H2O+HCl↽−−⇀H3O++Cl−

H3O+ oxidizes the magnesium to form the following equation
2H3O++Mg⟶Mg2++H2O+H2
Magnesium ions are formed and go into solution:
Rate=k⋅[H3O+]
Because it is the concentration of the H3O+ which determines the formation of the Mg ions.

From this, the rate law for the reaction is: Mg+2HCl⟶MgCl2+H2

Is merely: rate=k⋅[H3O+]

But [H3O+] is: [H3O+] = (K⋅[H2O][HCl])/[Cl−]
The rate law would be :
r=kobs×[H3O+]2=Aobsexp(Ea, obsRT)×[H3O+]2,
.

The hypothesis (es) we seek to test in this experiment is(are) ( what is the basis of your
experiment ):

The hypothesis is if the methods we've chosen to use yield an accurate result.

The key question the experiment seeks to a...

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Anonymous
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