3. A student conducts an experiment where she reacts a lump of zinc (Zn) with hydrochloric acid (HCl). The balanced equation below represents the reaction. Zn + 2HCl → H₂ + ZnCl₂ Which set of reaction conditions will produce H₂ at the fastest rate?*1.0 g of powdered Zn in 50mL of 1.0 M HCl at 20°Ca 1.0 g lump of Zn in 50mL of 0.5 M HCl at 30°C1.0 g of powdered Zn in 50mL of 1.0 M HCl at 30°Ca 1.0 g lump of Zn in 50mL of 0.5 M HCl at 20°C
Question
- A student conducts an experiment where she reacts a lump of zinc (Zn) with hydrochloric acid (HCl). The balanced equation below represents the reaction. Zn + 2HCl → H₂ + ZnCl₂ Which set of reaction conditions will produce H₂ at the fastest rate?*1.0 g of powdered Zn in 50mL of 1.0 M HCl at 20°Ca 1.0 g lump of Zn in 50mL of 0.5 M HCl at 30°C1.0 g of powdered Zn in 50mL of 1.0 M HCl at 30°Ca 1.0 g lump of Zn in 50mL of 0.5 M HCl at 20°C
Solution 1
The reaction conditions that will produce H₂ at the fastest rate would be "1.0 g of powdered Zn in 50mL of 1.0 M HCl at 30°C".
Here's why:
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Powdered Zn has a larger surface area than a lump of Zn, which allows for more collisions between reactant particles and thus a faster reaction rate.
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A higher concentration of HCl (1.0 M vs 0.5 M) means there are more HCl particles available to react with the Zn, which can also increase the reaction rate.
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A higher temperature (30°C vs 20°C) provides the particles with more energy, which can make collisions between particles more successful and thus increase the reaction rate.
Solution 2
The reaction conditions that will produce H₂ at the fastest rate would be "1.0 g of powdered Zn in 50mL of 1.0 M HCl at 30°C".
Here's why:
-
Powdered Zn has a larger surface area than a lump of Zn, which allows for more contact with the HCl and therefore a faster reaction rate.
-
A higher concentration of HCl (1.0 M vs 0.5 M) provides more reactant for the Zn to react with, which can also increase the reaction rate.
-
A higher temperature (30°C vs 20°C) increases the kinetic energy of the molecules, which makes them move faster and collide more often. This also increases the reaction rate.
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