Help: Zn and HCI reaction rate.

In summary, the chemical equation for the reaction between zinc and hydrochloric acid is Zn + 2HCl → ZnCl2 + H2. The rate of this reaction can be affected by factors such as concentration, temperature, surface area, and the presence of a catalyst. Increasing the concentration of reactants leads to a higher reaction rate, while increasing temperature leads to more frequent and energetic collisions and a higher reaction rate. A catalyst helps to lower the activation energy required for the reaction, allowing it to occur at a faster rate without being consumed in the process.
  • #1
Allergic2Chem
2
0
I need to check at what rate Zn and HCl react to release hydrogen gas.


How do I construct a hypothesis?

What method should I use?

What would the variables be? (independent, dependent, and controlled)

What relevance would all of this have to society?



Please help.


Allergic2Chem.
 
Physics news on Phys.org
  • #2
help? anyone?
 
  • #3
http://www.accessexcellence.org/LC/TL/filson/writhypo.php"

Hopefully, the rest follows from that.
 
Last edited by a moderator:

1. What is the chemical equation for the reaction between zinc and hydrochloric acid (HCI)?

The chemical equation for the reaction between zinc and hydrochloric acid is: Zn + 2HCl → ZnCl2 + H2.

2. What factors affect the rate of the zinc and HCI reaction?

The rate of the zinc and HCI reaction can be affected by concentration of reactants, temperature, surface area of the zinc, and presence of a catalyst.

3. How does concentration affect the reaction rate?

Increasing the concentration of reactants increases the frequency of collisions between particles, leading to a higher reaction rate.

4. What happens to the reaction rate as temperature increases?

As temperature increases, the particles have more kinetic energy and move faster, leading to more frequent and energetic collisions and a higher reaction rate.

5. What is the role of a catalyst in the zinc and HCI reaction?

A catalyst helps to lower the activation energy required for the reaction, allowing it to occur at a faster rate without being consumed in the process.

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