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In this experiment, we are investigating how the concentration of a reactant affects the rate of a chemical reaction. By using different concentrations of a solution and keeping all other variables the same, we can observe how quickly the reaction takes place at each concentration.

The rate of reaction is measured by how fast a product is formed (or how fast a reactant is used up). According to the collision theory, a higher concentration means more particles are present in the same volume, which leads to more frequent collisions between reacting particles. This should result in a faster reaction.

We will compare the rates by measuring the amount of product formed over time at different concentrations, helping us understand the effect of concentration on reaction rate.
Description (Magnesium + Hydrochloric Acid Reaction):
In this experiment, we are investigating how changing the concentration of hydrochloric acid affects the rate of reaction with magnesium ribbon. Hydrochloric acid reacts with magnesium to produce magnesium chloride and hydrogen gas:

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+
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→
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+
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+
2
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�Ѳ���(��)+2HCl (aq)→MgCl 2​(aq)+H 2(g)
We will use different concentrations of hydrochloric acid (e.g., 0.5M, 1.0M, 1.5M, 2.0M), while keeping other variables constant (e.g., volume of acid, temperature, and size of magnesium ribbon). As the reaction happens, hydrogen gas is released, and we will measure the volume of gas produced over time.

By comparing how quickly gas is produced at each concentration, we can determine how concentration affects the rate of reaction. A higher concentration is expected to produce gas more quickly, due to more frequent collisions between acid particles and magnesium, in line with collision theory.