Question

In lab, we put a piece of zinc in 50mL of 3M HCl, and there are 3 follow-up questions I don't know how to do it?
Table: Before the reaction:
-Mass of dry beaker 115.96g
-Mass of dry beaker+zinc 117.96g
After the reaction:
-Mass of dry beaker+zinc 117.38g
1. Suggest a reason why the reaction started very slowly then increased after a few minutes.
2. How would the results compare if twice the mass of zinc were used in this experiment?
3. a. How would the results compare if twice the amount of acid were added?
b. How would this affect the amount of

Answer 1

1- I would think that the piece of Zn has a layer of oxide because it spent some time in contact with air.
2-If twice the mass of Zn were used probably the reaction would proceed more slowly
3- If twice the amount of acid were added, the reaction would proceed faster because there is more reactant present.
I hope this helps!