Chlorine is toxic - Edexcel - GCSE Chemistry - Question 5 - 2020 - Paper 1
Question 5
Chlorine is toxic.
State one safety precaution that should be taken when using chlorine in the laboratory.
(b) Chlorine reacts with hydrogen to form hydrogen chlor... show full transcript
Worked Solution & Example Answer:Chlorine is toxic - Edexcel - GCSE Chemistry - Question 5 - 2020 - Paper 1
Step 1
State one safety precaution that should be taken when using chlorine in the laboratory.
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Answer
One safety precaution is to use a fume cupboard or fume hood to prevent inhalation of chlorine gas.
Step 2
Write the word equation for this reaction.
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Answer
Hydrogen + Chlorine → Hydrogen Chloride
Step 3
State what is seen when blue litmus paper is placed into this solution.
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Answer
The litmus paper turns red/pink, indicating the acidic nature of the solution.
Step 4
Complete the dot and cross diagram of a molecule of hydrogen chloride.
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Answer
In the dot and cross diagram, place one dot (●) to represent the hydrogen atom and a cross (✕) to represent the chlorine atom, connecting them with a line to show the bond.
Step 5
Name the type of bonding in a molecule of hydrogen chloride.
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The type of bonding in a molecule of hydrogen chloride is covalent bonding.
Step 6
Give a reason why this reaction occurs.
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The reaction occurs because chlorine is a more reactive halogen than bromine and displaces bromine from sodium bromide.
Step 7
State what would happen to the lamp when glucose solution is tested.
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The lamp would remain off because glucose is a non-electrolyte and does not conduct electricity.
Step 8
State what would happen to the lamp when sodium chloride solution is tested.
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The lamp would light up because sodium chloride dissociates into ions in solution, allowing it to conduct electricity.
Step 9
Describe how the conductivity of this solution changes as its concentration increases from 0 to 500 g dm-3.
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As the concentration increases from 0 to 150 g dm-3, the conductivity increases due to a greater number of ions in solution. However, beyond this point, e.g., at high concentrations, the conductivity may decrease due to ion pairing and saturation effects.
