Question 1

Which of the following metals will react most vigorously with hydrochloric acid ($$\mathrm{HCl}) to $$produce hydrogen gas?

Accepted Answer

Calcium ($$\mathrm{Ca})$$

Question 2

Given the activity series: $$\mathrm{Mg} \u003e \mathrm{Fe} \u003e \mathrm{Cu}$$, which of the following reactions will occur spontaneously?

Accepted Answer

$$\mathrm{Fe} + \mathrm{CuSO}_4 \rightarrow \mathrm{FeSO}_4 + \mathrm{Cu}$$

Question 3

Which observation would best indicate that a metal is reacting with an acid in a test tube?

Accepted Answer

A colorless gas is evolved and bubbles are seen.

Question 4

What is the net ionic equation for the reaction between magnesium metal and hydrochloric acid?

Accepted Answer

$$\mathrm{Mg}(s) + 2\mathrm{H}^+(aq) \rightarrow \mathrm{Mg}^{2+}(aq) + \mathrm{H}_2(g)$$

Question 5

A student adds zinc metal to a solution of copper(II) nitrate. Which of the following best describes what will happen?

Accepted Answer

Zinc will dissolve and copper metal will be deposited.

Question 6

Which of the following correctly lists the metals in order of decreasing reactivity based on the activity series provided in the study materials?

Accepted Answer

$$\mathrm{Ca} \u003e \mathrm{Mg} \u003e \mathrm{Zn} \u003e \mathrm{Fe} \u003e \mathrm{Cu}$$

Question 7

Which of the following reactions will NOT occur, based on the activity series?

Accepted Answer

$$\mathrm{Cu} + \mathrm{Zn(NO}_3)_2 \rightarrow \mathrm{Cu(NO}_3)_2 + \mathrm{Zn}$$

Question 8

In the reaction $$\mathrm{Mg}(s) + \mathrm{FeSO}_4(aq) \rightarrow \mathrm{MgSO}_4(aq) + \mathrm{Fe}(s)$$, which species is oxidized?

Accepted Answer

$$\mathrm{Mg}$$

Question 9

A piece of aluminum is placed in a solution of zinc nitrate. What is the correct net ionic equation for the reaction, if it occurs?

Accepted Answer

$$2\mathrm{Al}(s) + 3\mathrm{Zn}^{2+}(aq) \rightarrow 2\mathrm{Al}^{3+}(aq) + 3\mathrm{Zn}(s)$$

Question 10

Which of the following best explains why copper does not react with hydrochloric acid?

Accepted Answer

Copper is less reactive than hydrogen and cannot displace it from acid.

Question 11

A student observes that when magnesium is added to a solution of iron(II) sulfate, a gray solid forms and the solution changes color. What is the best explanation for this observation?

Accepted Answer

Magnesium is more reactive than iron and displaces it from solution.

Question 12

Which of the following is the correct molecular equation for the reaction between zinc and hydrochloric acid?

Accepted Answer

$$\mathrm{Zn}(s) + 2\mathrm{HCl}(aq) \rightarrow \mathrm{ZnCl}_2(aq) + \mathrm{H}_2(g)$$

Question 13

In the reaction $$2\mathrm{Fe}(s) + 3\mathrm{Cl}_2(g) \rightarrow 2\mathrm{FeCl}_3(s)$$, which species is the oxidizing agent?

Accepted Answer

$$\mathrm{Cl}_2(g)$$

Question 14

A student adds a piece of tin to a solution of copper(II) nitrate. What is the expected observation?

Accepted Answer

Tin dissolves and copper metal is deposited.

Question 15

Which of the following best describes the role of hydrogen in the reaction $$\mathrm{Zn}(s) + 2\mathrm{HCl}(aq) \rightarrow \mathrm{ZnCl}_2(aq) + \mathrm{H}_2(g)$$?

Accepted Answer

Hydrogen is reduced.

Question 16

Which of the following statements about the activity series is TRUE?

Accepted Answer

A metal higher in the activity series will displace a metal lower in the series from its salt solution.

Question 17

Which of the following is the correct net ionic equation for the reaction between iron and copper(II) sulfate solution?

Accepted Answer

$$\mathrm{Fe}(s) + \mathrm{Cu}^{2+}(aq) \rightarrow \mathrm{Fe}^{2+}(aq) + \mathrm{Cu}(s)$$

Question 18

A student places a piece of copper in a solution of magnesium nitrate. What will be observed?

Accepted Answer

No reaction will occur.

Question 19

Which of the following best explains why aluminum reacts slowly with hydrochloric acid, even though it is above hydrogen in the activity series?

Accepted Answer

Aluminum forms a protective oxide layer that slows the reaction.

Reactivity of Metals: Activity Series, Displacement Reactions, and Redox Equations - Lab 6

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