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IGCSE Sciences - Planning experiment, Exams of Chemistry

California Institute of Technology (Caltech)Chemistry

Hope this helps!~ Upvote so others can see this! All the best for you upcoming examinations! <3

Typology: Exams

2022/2023

Available from 05/05/2023

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Dr. Mohamed Gamal
3. Rusting
Q1.
Steps:
• Get an iron nail with 2g mass
• Get a test-tube and add 10 cm3 of tap water
• Place the iron nail in the test-tube and leave it to rust
• Observe the nail after a week
• Repeat the experiment using the other two water samples using
same volume of water and same surface area of nails and leave for
same time.
• compare the mass of the rusted nails and the largest change in mass
will have rusted the fastest
Q2.
Steps:
• Get a steel nail with 2g mass
• Add 10 cm3 of water and 5 cm3 of corrosion inhibitor R to a test-tube
• Place the nail in the test-tube and leave it for a week to rust
• Repeat this process with the inhibitors Q and S using same volumes
and duration (1 week) and same mass and surface area of the nail
• Compare the results, the nail with the least change in mass will have
the strongest corrosion inhibitor.
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3. Rusting

Q1.

Steps:

  • Get an iron nail with 2g mass
  • Get a test-tube and add 10 cm^3 of tap water
  • Place the iron nail in the test-tube and leave it to rust
  • Observe the nail after a week
  • Repeat the experiment using the other two water samples using same volume of water and same surface area of nails and leave for same time.
  • compare the mass of the rusted nails and the largest change in mass will have rusted the fastest

Q2.

Steps:

  • Get a steel nail with 2g mass
  • Add 10 cm^3 of water and 5 cm^3 of corrosion inhibitor R to a test-tube
  • Place the nail in the test-tube and leave it for a week to rust
  • Repeat this process with the inhibitors Q and S using same volumes and duration (1 week) and same mass and surface area of the nail
  • Compare the results, the nail with the least change in mass will have the strongest corrosion inhibitor.

5. Preparation of salts.

Q1.

  • Add dilute sulfuric acid to a beaker
  • Add excess magnesium oxide to the beaker
  • Heat the beaker on a Bunsen burner
  • Filter the excess unreacted magnesium oxide
  • Heat the solution (filtrate) till crystallization point , check for crystallization point by using a glass rod
  • Leave solution to cool
  • Filter crystals
  • Dry crystals gently using filter paper

6. Extraction of metals.

Q1.

Steps:

  • Crush malachite using mortar and pestle
  • Add nitric acid to the malachite
  • Solution is formed

1. Comparison between production of energy :

Q1:

Steps:

  • Add the first fuel (diesel) to spirit burner
  • Measure the Initial temperature of water
  • Start burn for certain time
  • Stop the reaction, Then Measure the Final temperature of water
  • Repeat experiment using the second fuel (biodiesel)
  • For fair comparison, use same volume of fuel/same volume of

water/same time interval/same distance between tube and

burner/same initial temperature

  • Fuel with greater temperature difference produce more energy.

Ideas for paper 6

(last question)

Q2 :

Steps:

  • Hold the test tube of water with stand & Put the peanuts below it
  • Measure the Initial temperature of water
  • Start burning for certain time
  • Stop the reaction, then Measure the Final temperature of water
  • Repeat the experiment with the other nuts (Brazil & hazel nuts)
  • For fair comparison, use same mass of nuts / same volume of water/ same distance between test tube and the nuts/ same initial temperature
  • Nuts with greater difference in temperature produce more energy. Q3:

Steps:

  • Use equal mass of coal , Crush it with mortar & pestle
  • Put the coal in fume cupboard and start heating
  • Pass it through potassium manganate(VII)
  • Then Measure Time taken for purple to become colourless
  • Repeat experiment with the second type of coal using same mass and same surface area
  • Coal with less time taken for colour to disappear produce most Sulfur dioxide.

Steps:

  • By Filteration
  • Sand in residue
  • Wash the residue & dry between two filter papers

4. How to determine:

Q1: The Concentraton:-

Steps:

  • Add 25 cm^3 of kleen up in flask
  • Add nitric acid to the burette
  • Add indicator to conical flask
  • Start adding acid to the flask until indicator change colour to neutral
  • Record volume of acid used
  • Then calculate the concentration:

No of moles of Ammonia = No of moles of nitric acid

C x V = C x V

Q2: The percentage :

Steps:

  • Weight the mixture (100g)
  • Add excess sulfuric acid
  • Warm and stir
  • Filter , wash and dry the residue (carbon) between filter paper
  • Then the mass of residue
  • Calculate the percentage :

100 – carbon mass

7. How to prepare an indicator :

Q1:

Steps :

  • Crush the berries with pestle and mortar
  • Add water and mix
  • Then filter off , the filtrate is the solution of an indicator

Q2:

Steps :

  • Add the indicator to hydrochloric acid
  • Add the indicator to sodium hydroxide
  • Colours must be different for each solution

11. Differentiate between 2 solutions :

Q1: Type of the solutions Steps :

  • Add x cm^3 of solution H to boiling tube
  • Add manganese(IV) oxide
  • Connect gas syringe to collect the gas
  • Start heating for certain time
  • Measure total volume of gas produced
  • Repeat the experiment with solution J using same volume of hydrogen peroxide and same mass of manganese(IV) oxide
  • Finally, the solution that produces large volume of oxygen gas is the new one. Q2: Strength of the solution: Steps :
  • Add 25 cm^3 of hydrochloric acid to a clean conical flask
  • Add few drops of methyl orange indicator into the conical flask
  • Fill the burette with oven cleaner C and note the starting volume
  • Start titration until the colour change
  • Then stop adding oven cleaner C and note the volume added
  • Repeat the experiment using same volume of oven cleaner B and same volume and concentration of HCl

8 .Reactivity Series :

Q1:

Steps:

  • Use 10 cm^3 of hydrochloric acid in test tube.
  • Add zinc metal.
  • Count the number of bubbles
  • Repeat experiment with silver and tin using same mass and surface area of metals.
  • The metal with the highest bubbles is the most reactive.

2. Catalyst:

Q1:

Steps:

  • Use same volume and concentration of hydrogen peroxide.
  • Add copper oxide to hydrogen peroxide.
  • Measure the volume of gas produced per unit time using a gas syringe.
  • Then compare that to the volume of gas produced from hydrogen peroxide without adding copper oxide.
  • Compare volume of gas produced

Q2:

Steps:

  • Weigh the copper oxide before adding to the hydrogen peroxide.
  • After the reaction is done, filter the copper oxide from the solution.
  • Dry it using an oven (or between two filter papers)
  • Weigh its mass
  • Compare the final mass with the initial mass.

10. Electroplating :

Q1:

Steps:

  • Prepare a copper sulfate solution.
  • Set up a circuit and a source of electricity.
  • Clean the ring using sand paper.
  • Place the ring at the cathode.
  • Place the copper rod in the anode.
  • Switch on electricity.
  • Make sure the ring is being rotated.
  • Remove the ring after electroplating and wash it.