EXPERIMENT 5: RATE OF DECOMPOSIT]ON OF HYDROGEN PEROXIDEPOTENTIAL HAZARDSSofety glosses must be worn...

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EXPERIMENT 5: RATE OF DECOMPOSIT]ON OF HYDROGEN PEROXIDE
POTENTIAL HAZARDS
Sofety glosses must be worn ot oll times in the lohoratory. Both H2O2 ond H2SOa qre strong oxidising
ogents ond shou!d not come into contact with your skin or, especiolly, eyes. Any offected skin should
be woshed continuously for XXXXXXXXXXmin under cold woter, while contaminoted clothing should be
removed ond washed thoroughly before reuse. Potossium permangonote is olso o strong oxidising
agent. lf spilled, wosh the offected oreas thoroughly.
NEVER PIPETTE SOLUTIONS MY MOUTH, ALWAYS USE THE PIPETTE FILLER PROVIDED.
INTRODUCTION
ln this experiment the first-order rate constant for the decomposition of hydrogen peroxide will be
determined.
The decomposition of hydrogen peroxide is a first-order reaction and occurs according to the
equation ...
Y
2H2O2(t) ) ZnrO(t)+ Oz(g)
The rate of decomposition is normally so small that evolution of oxygen gas is undetectable. The
reaction can be accelerated with the use of catalysts, such as finely divided MnO: or certain ions in
solution (e.g. Fe3*(aq), Mn2.(aq) and Bf(aq)).
For a first-order reaction the differential rate law states that
-otll=otot dt 1./
where -d[A]/dt is the rate of disappearance of reactant, [Aj is the amount of reactant remaining at
time t, k is the rate constant, and a is the stoichiometric coefficient of the reactant in the balanced
chemical equation, The initial concentration of reactant is designated [As].
lntegrating equation {1) gives
ln[A]= -kt + ln[Ao]
Hence a plot of ln[A] versus t should yield a straight line for a first order reaction with a slope equal
to -ak.
ln this experiment, Fe3*(aq) ions are used as the catalyst. The concentration of hydrogen peroxide at
any time will be determined by the titration of aliquots of the reaction solution with potassium
permanganate in acid solution.
(1)
(2-)
2Mnoo-(aq) + 5H2O2(aq)+ 6H*(aq) ) 2Mn2.(aq) + 5Oz(g)+ 8HrO(l)

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David · Accepted Answer

DECOMOSITION OF HYDROGEN PEROXIDE 
ABSTRACT:   
 Rate of a reaction is defined as the change in concentration of the 
reactants with respect to time. The unit of rate of a reaction is mol/L/s. Rate law 
equation is an equation that is used to relate the dependency of the rate of reaction 
on the concentration of the reactants. Thus, rate=k[conc]n, where n is the order of the 
reaction. Order is defined as the sum of the powers to which concentration terms are 
raised in the rate equation. N can be whole numbers, positive, negative or fractional. 
K is the rate constant of the reaction at a particular temperature.  Hydrogen 
peroxide is a compound that is used widely as an antiseptic, bleaching agent and 
disinfectant. It decomposes in presence of metal ion like Fe3+ to form water and 
oxygen. It is found that the reaction follows first order kinetics. The rate of the 
reaction generally decreases with the respect to time. The aim of this experiment is 
to study the rate of the reaction at different points of time and to determine the rate 
constant of the reaction. 
INTRODUCTION:  
Chemical Kinetics studies the speed of chemical reactions and the factors that 
influence the speed of a reaction. The speed of a chemical reaction is expressed ase 
reaction rate. The reaction rate is defined as the change in concentration of a 
reactant's or a product's concentration per unit time. It is defined such that 
irrespective of the choice of the reagent,  same rate is observed. 
For a general reaction, 
aA + bB  cC + dD  
where a,b,c,d refer to coefficients and the capital letters refer to reactants 
and products, the reaction rate is defined as:
The Δ refers to the change in the quantity after it and equals the final value 
of the quantity minus the initial value of the quantity. For example, Δ [A] = 
[A]final – [A]initial and Δ t = tfinal – tinitial. The reaction rate is defined so that it is 
always a positive quantity. The equations with reactants have negative 
signs in front of them to ensure that the reaction rate is positive, as 
reactants decrease with respect to time. Reaction rates will have units of 
concentration per unit time, such as M s
-1
 or mol L
-1
 min
-1
. 
Experimentally,

EXPERIMENT 5: RATE OF DECOMPOSIT]ON OF HYDROGEN PEROXIDE POTENTIAL HAZARDS Sofety glosses must be worn ot oll times in the lohoratory. Both H2O2 ond H2SOa qre strong oxidising ogents ond shou!d not...

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