Multiple choice questions

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For some of these questions, you need data from the appendices of Inorganic Chemistry, third edition by C.E. Housecroft and A.G. Sharpe. On opening the book cover you will find a periodic table and a list of elements and atomic masses. Physical constants are listed on the back inside cover of the book.

Multiple choice questions by Catherine E. Housecroft

This activity contains 20 questions.

In which of the following is the metal reduced? (These are not balanced equations.)

	[Fe(CN)₆]^4– → [Fe(CN)₆]^3–
	[MnO₄]^– → MnO₂
	[MnO₄]^2– → [MnO₄]^–
	[Cr₂O₇]^2– → [CrO₄]^2–

For the cell: 2Ag⁺(aq) + Zn(s) →2Ag(s) + Zn²⁺(aq)
E^o _cell = 1.56 V. The value of ΔG^o is:

	–150 kJ per mole of Zn
	–602 kJ per mole of Ag
	–301 kJ per mole of Ag
	–301 kJ per mole of Zn

If ΔG^o(350 K) = –72 kJ mol^–1, the value of K is:

	5.6 x 10¹⁰
	4.2 x 10¹²
	5.5 x 10²⁴
	1.2 x 10²⁹

For a thermodynamically spontaneous cell reaction, which statement is correct?

	E^o (reduction) must be more negative than E^o (oxidation)
	E^o (oxidation) must be more negative than E^o (reduction)
	E^o_cell should be negative
	The difference between E^o (reduction) and E^o (oxidation) must be more than 1.0 V

Use Appendix 11 in Inorganic Chemistry to determine E^o_cell for the reaction: Cl₂ + 2Br^– →2Cl^– + Br₂. The value is:

	–2.45 V
	–0.27 V
	0.27 V
	2.45 V

Use Appendix 11 in Inorganic Chemistry for this question. For a Cu²⁺(aq) / Cu(s) half-cell (at 298 K) in which [Cu²⁺] = 0.02 mol dm^–3, E is:

	+0.44 V
	+0.39 V
	+0.29 V
	+0.24 V

pH affects the E value for:

	the reduction of [Cr₂O₇]^2– to Cr³⁺
	the reduction of Cr³⁺ to Cr²⁺
	the reduction of Cr²⁺ to Cr
	the reduction of Cr³⁺ to Cr

Look at Figure 8.2 in Inorganic Chemistry. In alkaline solution, the value of E^o (at pH 14) for the reduction of [MnO₄]^– to Mn(OH)₂ is:

	+0.63 V
	+0.55 V
	+0.34 V
	+1.69 V

Look at Figure 8.6 in Inorganic Chemistry. Carbon will reduce FeO to Fe at:

	1500 K
	900 K
	700 K
	500 K

Δ_solG^o for KBr can be calculated using the equation:

	Δ_fG^o (K⁺,g) + Δ_fG^o (Br^–,g) – Δ_fG^o (KBr,s)
	–Δ_fG^o (K⁺,g) – Δ_fG^o (Br^–,g) – Δ_fG^o (KBr,s)
	Δ_fG^o (K⁺,aq) + Δ_fG^o (Br^–,aq) + Δ_fG^o (KBr,s)
	Δ_fG^o (K⁺,aq) + Δ_fG^o (Br^–,aq) – Δ_fG^o (KBr,s)

Look at Figure 8.4a in Inorganic Chemistry. Which species, if any, is thermodynamically unstable with respect to disproportionation at pH 0?

	No species
	Cr²⁺
	Cr³⁺
	[Cr₂O₇]^2–

Using data in Appendix 11 in Inorganic Chemistry, choose which statement is true.

	On going from [Fe(OH₂)₆]ⁿ⁺ to [Fe(phen)₃]ⁿ⁺, Fe(II) is stabilized with respect to oxidation to Fe(III)
	On going from [Fe(OH₂)₆]ⁿ⁺ to [Fe(bpy)₃]ⁿ⁺ (n = 2 or 3), Fe(III) is stabilized with respect to reduction to Fe(II)
	On going from [Fe(OH₂)₆]ⁿ⁺ (n = 2 or 3) to [Fe(CN)₆]^n– (n = 3 or 4), Fe(II) is stabilized with respect to oxidation to Fe(III)
	On going from [Fe(OH₂)₆]ⁿ⁺ to [Fe(phen)₃]ⁿ⁺ (n = 2 or 3), Fe(III) is stabilized with respect to reduction to Fe(II)

In which of the following species is N in the highest oxidation state?

	N₂O₅
	[NH₄]⁺
	NO₂
	[NO₂]^–

Consider the following reaction:

Au + O₂ + 3F₂ → [O₂]⁺[AuF₆]^–

Which statement is correct about the redox changes in this reaction?

	Au is oxidized; O is oxidized; F is reduced
	Au is reduced; O is oxidized; F is reduced
	Au is oxidized; O does not undergo a redox change; F is reduced
	Au is reduced; O is oxidized; F is oxidized

Use data in Appendix 11 of Inorganic Chemistry to determine a value for ΔG^o(298 K) per mole of Fe²⁺ for the reaction:

[Cr₂O₇]^2– + 14H⁺ + 6Fe²⁺ → 2Cr³⁺ + 6Fe³⁺ + 7H₂O

	–54 kJ mol^–1
	–324 kJ mol^–1
	–1216 kJ mol^–1
	–203 kJ mol^–1

A potential diagram for iodine at pH 0 shows the following E^o values:
[IO₃]^- → HOI E^o = +1.14 V
[IO₃]^- → I₂ E^o = +1.20 V
What is the value of E^o for the reduction of HOI to I₂?

	+1.24 V
	+0.06 V
	+1.44 V
	+1.56 V

In neutral aqueous solution, E^o for the Mn³⁺/Mn²⁺ couple is +1.54 V. At pH 14, E^o for the Mn(OH)₃/Mn(OH)₂ couple is +0.15 V. Which of the following statements is incorrect?

	At pH 14, Mn(II) and Mn(III) both precipitate from aqueous solution as hydroxides
	Mn(III) is less stable with respect to reduction to Mn(II) at pH 14 than at pH 7
	The Mn(OH)₃/Mn(OH)₂ couple refers to an equilibrium involving Mn(III) and Mn(II)
	At pH 7, Mn³⁺(aq) is a relatively strong oxidizing agent

Which factor below does not contribute to the value of the standard reduction potential for the process: Na⁺(aq) + e^- → Na(s)

	Enthalpy change for electron attachment to Na(g)
	Enthalpy change for atomization of Na(s)
	First ionization energy of Na(g)
	Enthalpy change for hydration of Na(g)

Which of the following reactions is an example of disproportionation?

	2NO₂ + H₂O → HNO₂ + HNO₃
	4HNO₃ → 4NO₂ + O₂ + 2H₂O
	3Cu + 8HNO₃→ 3Cu(NO₃)₂ + 4H₂O + 2NO
	2NO + O₂ → 2NO₂

A potential diagram for rhenium at pH 0 shows the following E^o values:
[ReO₄]^- → ReO₂ E^o = +0.51 V
ReO₂ → Re³⁺ E^o = +0.16 V
Re³⁺ → Re E^o = +0.30 V
The value of E^o for the reduction of [ReO₄]^- to Re(0) is:

	+0.97 V
	+0.32 V
	+0.14 V
	+0.37 V

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