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A 2.0 g piece of magnesium ribbon was added to a known volume of 2.0 M hydrochloric acid - VCE - SSCE Chemistry - Question 1 - 2008 - Paper 1
Question 1
A 2.0 g piece of magnesium ribbon was added to a known volume of 2.0 M hydrochloric acid. The volume of hydrogen gas produced during the reaction was measured and re... show full transcript
Worked Solution & Example Answer:A 2.0 g piece of magnesium ribbon was added to a known volume of 2.0 M hydrochloric acid - VCE - SSCE Chemistry - Question 1 - 2008 - Paper 1
Step 1
Write an equation for the reaction between magnesium and hydrochloric acid.
Answer
The balanced chemical equation for the reaction between magnesium and hydrochloric acid is:
This equation shows that one mole of magnesium reacts with two moles of hydrochloric acid to produce one mole of magnesium chloride and one mole of hydrogen gas.
Step 2
In a second experiment, 2.0 g of magnesium powder was added to the same volume of 2.0 M hydrochloric acid as used in the first experiment.
Answer
In this case, since magnesium powder has a greater surface area compared to magnesium ribbon, the reaction will occur more rapidly, resulting in a faster production of hydrogen gas.
Graph Explanation:
- The graph should start at the origin and rise steeply at first, indicating a rapid production of hydrogen gas due to the increased reactivity of powdered magnesium.
- As the reaction proceeds, the slope will decrease, showing a slower rate of hydrogen production as the magnesium powder gets consumed.
- Finally, the graph will plateau when all the magnesium has reacted, indicating that the hydrogen gas production has ceased.
Expected Graph:
- The graph will be a curve that rises steeply at first, gradually leveling off.