The balanced equation below represents the reaction between a 5.0 gram sample of zinc metal and 0.5 m of hydrochloric acid. the reaction takes place in an open test tube at 298k and 1 atm in a laboratory activity

1) Increasing the concentration of HCl [HCl] will increase the reaction rate.

2) The potential energy diagram is shown in the attached image.

3) Because of it is an irreversible reaction that goes to the forward direction . The reaction takes place till HCl dissolves Zn completely.

Explanation:

Q1: State one change in reaction conditions, other than adding catalyst, that will increase the rate of the reaction.

Rate = k[HCl]².

Rate ∝ [HCl]².

So, increasing the concentration of HCl [HCl] will increase the reaction rate.

Q2: Draw a potential energy diagram for this reaction.

In an exothermic reaction, the energy of the reactants is higher than that of the products.

The potential energy diagram is shown in the attached image.

Q3: Explain why this reaction will not reach equilibrium.

Because of it is an irreversible reaction that goes to the forward direction . The reaction takes place till HCl dissolves Zn completely.

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)