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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 reaction between magnesium and hydrochloric acid can be represented by the following balanced chemical equation:
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
Sketch the expected graph of volume of hydrogen against time for this second experiment.
Answer
In the second experiment, when magnesium powder is added, the surface area of magnesium available for reaction is greater than that of the ribbon. Therefore, I expect the volume of hydrogen gas produced to increase at a faster rate initially.
The expected graph would appear as follows:
- A steep curve indicating a rapid release of hydrogen gas at the beginning due to the increased surface area of the magnesium powder.
- The curve would then begin to level off as the magnesium is consumed and the reaction slows down, leading to less hydrogen gas produced over time.
In summary, the expected graph would start with a steep incline, followed by a gradual leveling off as the reaction progresses. This indicates a faster reaction rate compared to the ribbon due to the increased surface area.