Berry List of Chemistry Experiments (PEKA) Form 5 (Part 1)

by BerryBerryTeacher

in Berry Experiment (Experiments & PEKA)

This post is the list of PEKA experiments for SPM Chemistry Form 5 from Berry Berry Easy. Please familiarise with all these experiments from Form 5 Chemistry Chapter 1: Rate of Reactions before conducting them so as to be better prepared. The list of experiments are as below:

Berry List of Chemistry Experiments (PEKA) Form 5 (Part 1)

Chapter 1 – Rate of Reactions

List of PEKA experiments:

  1. Average rate of reaction and instantaneous rate of reaction
  2. Effect of surface area on the rate of reaction
  3. Effect of concentration on the rate of reaction
  4. Effect of temperature on the rate of reaction
  5. Effect of catalyst on the rate of reaction
  6. Effect of the amount of catalyst on the rate of reaction
Number Laboratory Work 1.2
Pg. 3
Title Average rate of reaction and instantaneous rate of reaction
Aim To determine the average rate of reaction and the instantaneous rate of reaction
Apparatus
  • 50 cm3 beaker
  • Test tube
  • Spatula
Material
  • Marble chip
  • 2.0  mol dm-3 hydrochloric acid (HCl)
  • 0.1 mol dm-3 sodium thiosulphate, Na2S2O3 solution
  • 1.0 mol dm-3 lead(II) nitrate solution

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Number Experiment 1.1
Pg. 6
Title Effect of surface area on the rate of reaction
Aim To investigate the effect of total surface area of the reactant on the rate of reaction
Problem Statement How does the total exposed surface area of a solid reactant affect the rate of reaction?
Hypothesis When the total surface area of marble chips increases, the rate of reaction increases. / The smaller the size of the reactant particles, that is, the larger the total surface area of the reactant particles, the higher the rate of reaction.
Apparatus
  • 50 cm3 measuring cylinder
  • 150 cm3 conical flask
  • Stopper with delivery tube
  • Basin
  • Burette
  • Spatula
  • Electronic balance
  • Stopwatch
Material
  • 0.5 mol dm-3 hydrochloric acid (HCl)
  • 2 g large marble chips
  • 2 g small marble chips
  • Water
Variables
  • Manipulated variable: Total surface area of marble chips
  • Responding variable: Rate of reaction
  • Controlled / Fixed variable: Mass of marble chips, volume and concentration of hydrochloric acid (HCl), temperature
Operational Definition
  • 1. Smaller marble chips have a larger total surface area than larger marble chips of the same mass.
  • 2. For the graph of the volume of gas released against time, the curve with higher initial gradient indicates a higher initial rate of reaction.

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Number Experiment 1.2
Pg. 10
Title Effect of concentration on the rate of reaction
Aim To investigate the effect of concentration on the rate of reaction
Problem Statement How does the concentration of a reactant affect the rate of reaction? / Does high concentration of sodium thiosulphate Na2S2O3 solution decrease the time taken for the mark ‘X’ to disappear from sight?
Hypothesis When the concentration of sodium thiosulphate, Na2S2O3 solution increases, the rate of reaction increases. / The higher the concentration of sodium thiosulphate Na2S2O3 solution, the shorter the time taken for the mark ‘X’ to disappear from sight.
Apparatus
  • 150 cm3 conical flask
  • 50 cm3 measuring cylinder
  • 10 cm3 measuring cylinder
  • Stopwatch
Material
  • 0.2 mol dm-3 sodium thiosulphate solution
  • 1.0 mol dm-3 sulphuric acid
  • Distilled water
  • White paper marked ‘X’ at the centre
Variables
  • Manipulated variable:  Concentration of sodium thiosulphate, Na2S2O3 solution
  • Responding variable: Rate of reaction
  • Controlled / Fixed variable: Concentration, volume and initial temperature of sulphuric acid, H2SO4. Total volume of reactants
Operational Definition Rate of reaction is inversely proportional to the time taken for the the mark ‘X’ to disappear from sight

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Number Experiment 1.3
Pg. 13
Title Effect of temperature on the rate of reaction
Aim To investigate the effect of temperature on the rate of reaction
Problem Statement How does temperature affect the rate of reaction?
Hypothesis An increase in temperature will increase the rate of reaction.
Apparatus
  • 150 cm3 conical flask
  • 50 cm3 measuring cylinder
  • 10 cm3 measuring cylinder
  • Stopwatch
  • Thermometer
  • Bunsen burner
  • Tripod stand
  • Wire gauze
Material
  • 0.2 mol dm-3 sodium thiosulphate solution
  • 1.0 mol dm-3 sulphuric acid
  • White paper marked ‘X’ at the centre
Variables
  • Manipulated variable: Temperature of sodium thiosulphate, Na2S2O3 solution
  • Responding variable: The time taken for the cross ‘X’ to disappear
  • Controlled / Fixed variable: volume and concentration of sodium thiosulphate Na2S2O3 solution, volume and concentration of sulphuric acid, size of conical flask
Operational Definition Rate of reaction is inversely proportional to the time taken for the mark ‘X’ to disappear from sight

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Number Experiment 1.4
Pg. 15
Title Effect of catalyst on the rate of reaction
Aim To investigate the effect of a catalyst on the rate of reaction
Problem Statement How does a catalyst affect the rate of reaction? / How do catalysts affect the rate of decomposition of hydrogen peroxide?
Hypothesis The presence of a catalyst increases the rate of reaction. / Manganese(IV) oxide increases the rate of decomposition of hydrogen peroxide.
Apparatus
  • Test tube
  • Test tube rack
  • Spatula
  • Wooden splinter
  • Retort stand and clamp
  • 10 cm3 measuring cylinder
  • Electronic balance
  • Weighing bottle
Material
  • 20-volume hydrogen peroxide, H2O2 solution
  • 1.0 g Manganese(IV) oxide powder
Variables
  • Manipulated variable: Presence or absence of a catalyst
  • Responding variable: The release of oxygen gas / Rate of reaction
  • Controlled / Fixed variable: Volume  and concentration of hydrogen peroxide (H2O2) solution, temperature
Operational Definition
  • The decomposition of hydrogen peroxide is fast if the glowing wooden splinter rekindles brightly and rapidly.
  • The decomposition of hydrogen peroxide is slow if the glowing wooden splinter glows dimly and slowly.

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Number Experiment 1.5
Pg. 17
Title Effect of the amount of catalyst on the rate of reaction
Aim To investigate the effect of the amount of catalyst on the rate of reaction.
Problem Statement How does the amount of a catalyst affect the rate of reaction?  / Does higher amount of catalysts increases the rate of reaction?
Hypothesis When the amount of a catalyst used increases, the rate of reaction increases. / The higher the amount of the catalysts, the higher the rate of reaction.
Apparatus
  • 50 cm3 measuring cylinder
  • 150 cm3 conical flask
  • Stopper with delivery tube
  • Burette
  • Retort stand and clamp
  • Basin
  • Stopwatch
  • Electronic balance
  • Spatula
  • Weighing bottle
  • Beakers
Material
  • 2-volume hydrogen peroxide solution
  • 1.0 g manganese(IV) oxide powder
Variables
  • Manipulated variable: amount / mass of catalyst
  • Responding variable: Rate of reaction
  • Controlled / Fixed variable: Temperature, volume and concentration of hydrogen peroxide solution
Operational Definition The curves for the graph of volume of gas liberated against time a higher gradient indicated a higher rate of reaction.

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January 15, 2013
January 24, 2013

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