DP Chemistry Questionbank

• Syllabus

Topic 19: Redox processes

Sub sections and their related questions

19.1 Electrochemical cells

• 15M.1.hl.TZ1.31: Two half-cells are connected via a salt bridge to make a voltaic cell. Which statement about this...
• 15M.1.hl.TZ1.32: Which signs are correct for a spontaneous redox reaction?
• 15M.1.hl.TZ1.33: Consider the standard electrode...
• 15M.1.hl.TZ2.32: The standard electrode potentials for three reactions involving copper and copper ions are:     ...
• 15M.1.hl.TZ2.33: The same quantity of electricity is passed through separate dilute aqueous solutions of sulfuric...
• 15M.2.hl.TZ1.6d.ii: Predict the products formed at the electrodes during the electrolysis of concentrated aqueous...
• 15M.2.hl.TZ1.6f.i: Define the term standard electrode potential, \({E^\Theta }\).
• 15M.2.hl.TZ1.6f.ii: Draw a labelled diagram for the voltaic cell in which the following reaction...
• 15M.2.hl.TZ2.8e.i: Define the term standard electrode potential.
• 15M.2.hl.TZ2.8e.iii: Predict the balanced equation for the spontaneous reaction which will produce a current in this...
• 15M.2.hl.TZ2.8e.iv: Identify the negative and the positive electrodes in this cell.
• 15M.2.hl.TZ2.8e.v: Predict the direction of movement of electrons in the external circuit.
• 15M.2.hl.TZ2.8e.vi: State the directions in which the negative ions (anions) and the positive ions (cations) flow in...
• 14M.1.hl.TZ1.33: The overall equation of a voltaic cell...
• 14M.1.hl.TZ2.33: Which components are used to make the standard hydrogen electrode? A.    ...
• 14M.1.hl.TZ2.34: What is the cell potential, in V, of the reaction...
• 14M.2.hl.TZ1.6b: (i)     Deduce the order of reactivity of these four metals, from the least to the most...
• 14M.2.hl.TZ1.6c: (i)     State the half-equation for the reaction that occurs at each electrode.   Positive...
• 14M.2.hl.TZ1.6d: (i)     Determine the mass of copper produced at one of the electrodes in cell 2 if the tin...
• 14M.2.hl.TZ2.8g: (i)     Draw a labelled diagram of a suitable apparatus for the electrolysis.   (ii)     State...
• 14N.1.hl.TZ0.32: Consider the following standard electrode potentials.     ...
• 14N.1.hl.TZ0.33: A number of molten metal chlorides are electrolysed, using the same current for the same length...
• 14N.2.hl.TZ0.10f: (i)     An aqueous solution of sodium chloride is electrolysed using inert electrodes. Explain...
• 14N.2.hl.TZ0.10g: Describe how electrolysis can be used to electroplate a bracelet with a layer of silver metal....
• 13N.1.hl.TZ0.33: Consider the following two standard electrode potentials at 298 K.     ...
• 13N.1.hl.TZ0.34: What happens during the electrolysis of concentrated aqueous potassium chloride? I.   ...
• 13N.2.hl.TZ0.6a: Define the term standard electrode potential, \({E^\Theta }\).
• 13N.2.hl.TZ0.6c: In the two experiments below, predict whether a reaction would occur and deduce an equation for...
• 13N.2.hl.TZ0.6d.i: Using Table 14 of the Data Booklet, state the balanced half-equation for the reaction that occurs...
• 13N.2.hl.TZ0.6d.ii: Calculate the cell potential in V.
• 13N.2.hl.TZ0.6d.iii: On the diagram above label with an arrow • the direction of electron flow in the wire • the...
• 13M.1.hl.TZ1.31: An aqueous solution of a metal salt is electrolysed. Which factor will have no effect on the mass...
• 13M.1.hl.TZ1.33: The standard electrode potentials of some half-reactions are given below.     ...
• 13M.2.hl.TZ1.4e.ii: Explain the sign of the calculated standard electrode potential.
• 13M.2.hl.TZ1.4f: Predict the sign of \(\Delta {G^\Theta }\) for this reaction.
• 13M.2.hl.TZ1.7c.iii: Predict and explain the products of electrolysis of a dilute iron(II) bromide solution.
• 13M.2.hl.TZ1.7c.iv: Identify another product that is formed if the solution of iron(II) bromide is concentrated.
• 13M.2.hl.TZ1.7c.v: Explain why this other product is formed.
• 13M.1.hl.TZ2.32: Which statement is correct for electroplating an object with gold? A.     The object must be the...
• 13M.2.hl.TZ2.7c.i: Describe the standard hydrogen electrode including a fully labelled diagram.
• 13M.2.hl.TZ2.7c.ii: Define the term standard electrode potential, \({E^\Theta }\).
• 13M.2.hl.TZ2.7d.ii: Using Table 14 of the Data Booklet, calculate the cell potential, \(E_{{\text{cell}}}^\Theta \),...
• 13M.2.hl.TZ2.7e.i: Deduce the sign of the standard free energy change, \(\Delta {G^\Theta }\), for any...
• 13M.2.hl.TZ2.7e.ii: State why dilute sulfuric acid needs to be added in order for the current to flow in the...
• 13M.2.hl.TZ2.7e.iii: State why copper electrodes cannot be used in the electrolysis of water. Suggest instead suitable...
• 13M.2.hl.TZ2.7e.iv: Deduce the half-equations for the reactions occurring at the positive electrode (anode) and the...
• 13M.2.hl.TZ2.7e.v: Deduce the overall cell reaction, including state symbols.
• 13M.2.hl.TZ2.7e.vii: Comment on what is observed at both electrodes.
• 13M.2.hl.TZ2.7f: Two electrolytic cells are connected in series (the same current passes through each cell). One...
• 13M.1.sl.TZ2.25: The overall reaction in the voltaic cell below is: Which statement is correct for the nickel...
• 12N.2.hl.TZ0.4b: (i)     Draw an annotated diagram of the electrolytic cell in process 1 and identify the...
• 10N.1.hl.TZ0.32: A voltaic cell is made by connecting two half-cells represented by the half-equations...
• 10N.1.hl.TZ0.33: For the electrolysis of aqueous copper(II) sulfate, which of the following statements is...
• 10N.2.hl.TZ0.4b: (i)     Explain how molten magnesium chloride conducts an electric current. (ii)     Identify...
• 09N.1.hl.TZ0.31: Which are necessary conditions for the standard hydrogen electrode to have an \({E^\Theta }\) of...
• 09N.2.hl.TZ0.4b.i: Deduce a balanced equation for the overall reaction which will occur spontaneously when these two...
• 09N.2.hl.TZ0.4b.ii: Determine the cell potential when the two half-cells are connected.
• 10M.2.hl.TZ1.6a.iii: Using Table 14 of the Data Booklet, calculate the cell potential for this cell.
• 10M.2.hl.TZ1.6b: The standard electrode potentials for three other electrode systems are given below. (i)   ...
• 10M.2.hl.TZ1.6c: These values were obtained using a standard hydrogen electrode. Describe the materials and...
• 10M.2.hl.TZ1.6d.iii: Two electrolytic cells are connected in series as shown in the diagram below. In one there is...
• 10M.3.hl.TZ1.C3: Discuss the production of chlorine and sodium hydroxide from brine using a membrane cell. Include...
• 10M.2.hl.TZ2.8b: (i)     Molten sodium chloride is electrolysed in a cell using inert electrodes. State the...
• 10M.2.hl.TZ2.8c: Electroplating is an important application of electrolytic cells with commercial implications....
• 09M.1.hl.TZ1.32: Consider these standard electrode...
• 09M.2.hl.TZ1.7a.i: Define the term standard electrode potential and state the meaning of the minus sign in the value...
• 09M.2.hl.TZ1.7a.ii: Calculate the value for the standard electrode potential for the cobalt half-cell.
• 09M.2.hl.TZ1.7a.iv: Deduce the equation for the spontaneous reaction taking place when the iron half-cell is...
• 09M.2.hl.TZ1.7a.v: Explain the function of the salt bridge in an electrochemical cell.
• 09M.2.hl.TZ1.7c.i: Draw a labelled diagram of the cell. Use an arrow to show the direction of the electron flow and...
• 09M.2.hl.TZ1.7c.ii: Give the formulas of all the ions present in the solution.
• 09M.2.hl.TZ1.7c.iii: Predict the products obtained at each electrode and state the half-equation for the formation of...
• 09M.2.hl.TZ1.7c.iv: Deduce the molar ratios of the products obtained at the two electrodes.
• 09M.2.hl.TZ1.7d.i: concentrated sodium chloride
• 09M.1.hl.TZ2.32: What is the cell potential, in V, for the reaction that occurs when the following two half-cells...
• 09M.2.hl.TZ2.6c.v: Electroplating is an important application of electrolysis. State the composition of the...
• 11M.2.hl.TZ1.9a.ii: Deduce the equations for the formation of the major product at the positive electrode (anode)...
• 11M.2.hl.TZ1.9b.i: Use Table 14 of the Data Booklet to deduce the equation for the spontaneous reaction occurring in...
• 11M.2.hl.TZ1.9b.ii: Calculate the standard potential for this cell.
• 11M.2.hl.TZ1.9b.iii: State the conditions necessary for the potential of the cell to equal that calculated in part (b)...
• 11M.2.hl.TZ1.9c: Using the data below and data from Table 14 of the Data Booklet, predict and explain which metal,...
• 11M.2.hl.TZ1.9d.i: Electrolysis is used in the electroplating of metals. The same amount of current is passed...
• 11M.2.hl.TZ1.9d.ii: For the \({\text{Sn(S}}{{\text{O}}_{\text{4}}}{{\text{)}}_{\text{2}}}\) cell, suggest two...
• 11M.1.hl.TZ2.32: The standard electrode potentials for two metals are given...
• 11M.1.hl.TZ2.33: The same quantity of electricity was passed through separate molten samples of sodium bromide,...
• 11M.2.hl.TZ2.7a.i: Define standard electrode potential.
• 11M.2.hl.TZ2.7a.ii: Explain the significance of the minus sign in \( - {\text{0.45 V}}\).
• 11M.2.hl.TZ2.7b.i: State the species which is the strongest oxidizing agent.
• 11M.2.hl.TZ2.7b.ii: Deduce which species can reduce \({\text{S}}{{\text{n}}^{4 + }}{\text{(aq)}}\) to...
• 11M.2.hl.TZ2.7b.iii: Deduce which species can reduce \({\text{S}}{{\text{n}}^{2 + }}{\text{(aq)}}\) to Sn(s) under...
• 11M.2.hl.TZ2.7c.i: Draw a labelled diagram of a voltaic cell made from an Fe (s) /...
• 11M.2.hl.TZ2.7c.ii: Deduce the equation for the chemical reaction occurring when the cell in part (c) (i) is...
• 11M.2.hl.TZ2.7e.ii: Explain why an aqueous solution of sodium chloride cannot be used to obtain sodium metal by...
• 12M.1.hl.TZ2.30: Consider the following standard electrode...
• 12M.1.hl.TZ2.31: Two electrolytic cells are connected in series and the same current passes through each cell. The...
• 11N.1.hl.TZ0.31: Four electrolytic cells are constructed. Which cell would produce the greatest mass of metal at...
• 11N.2.hl.TZ0.7d.i: Draw a diagram of the voltaic cell, labelling the positive and negative electrodes (cathode and...
• 11N.2.hl.TZ0.7d.ii: Define the term standard electrode potential.
• 11N.2.hl.TZ0.7d.iii: Calculate the cell potential, in V, under standard conditions, using information from Table 14 of...
• 11N.2.hl.TZ0.7f: Chromium is often used in electroplating. State what is used as the positive electrode (anode),...
• 16M.1.hl.TZ0.32: Which...
• 16M.1.hl.TZ0.33: z mol...
• 16M.2.hl.TZ0.4b: Tin can also exist in the +4 oxidation state. Vanadium can be reduced from an oxidation state...
• 16N.1.hl.TZ0.32: Which signs for both Eθcell and ΔGθ result in a spontaneous redox reaction occurring under...
• 16N.1.hl.TZ0.33: An iron rod is electroplated with silver. Which is a correct condition for this process? A. The...
• 16N.2.hl.TZ0.4i: Magnesium chloride can be electrolysed. (i) Deduce the half-equations for the reactions at each...
• 16N.2.hl.TZ0.4j: Standard electrode potentials are measured relative to the standard hydrogen electrode. Describe...
• 16N.2.hl.TZ0.4k: A magnesium half-cell, Mg(s)/Mg2+(aq), can be connected to a copper half-cell,...
• 16N.3.hl.TZ0.21b: A concentration cell is an example of an electrochemical cell. (i) State the difference between...
• 17M.1.hl.TZ1.30: Which statement is correct for the overall reaction in a voltaic cell? 2AgNO3(aq) + Ni(s) →...
• 17M.1.hl.TZ1.31: In the electrolysis of aqueous potassium nitrate, KNO3(aq), using inert electrodes, 0.1 mol of a...
• 17M.2.hl.TZ1.3b.i: Identify, from the table, a non-vanadium species that can reduce VO2+(aq) to V3+(aq) but no further.
• 17M.2.hl.TZ1.3b.ii: Identify, from the table, a non-vanadium species that could convert...
• 17M.2.hl.TZ1.3c.ii: Comment on the spontaneity of this reaction by calculating a value for \(\Delta {G^\theta...
• 17M.1.hl.TZ2.30: What is the standard half-cell potential of copper if the “zero potential reference electrode”...
• 17M.1.hl.TZ2.31: What are the relative volumes of gas given off at E and F during electrolysis of the two cells...
• 17M.2.hl.TZ2.2b.i: Corrosion of iron is similar to the processes that occur in a voltaic cell. The initial steps...
• 17M.2.hl.TZ2.2b.ii: Calculate the Gibbs free energy, ΔG θ, in kJ, which is released by the corrosion of 1 mole of...
• 17M.2.hl.TZ2.2c: Zinc is used to galvanize iron pipes, forming a protective coating. Outline how this process...
• 17N.1.hl.TZ0.31: What are the products when an aqueous solution of copper(II) sulfate is electrolysed using...
• 17N.2.hl.TZ0.7b: Predict, giving a reason, the direction of movement of electrons when the standard nickel and...
• 17N.2.hl.TZ0.7c: Calculate the cell potential, in V, when the standard iodine and manganese half-cells are connected.
• 17N.2.hl.TZ0.7e: State and explain the products of electrolysis of a concentrated aqueous solution of sodium...
• 18M.1.hl.TZ1.30: Which combination would electroplate an object with copper?
• 18M.1.hl.TZ1.31: What does not affect the mass of products formed in electrolysis of an aqueous solution? A.   ...
• 18M.2.hl.TZ1.6d: Calculate the cell potential, in V, using section 24 of the data booklet.
• 18M.2.hl.TZ1.6e: Determine the loss in mass of one electrode if the mass of the other electrode increases by 0.10 g.
• 18M.1.hl.TZ2.30: Two cells undergoing electrolysis are connected in series. If \(x\) g of silver are deposited...
• 18M.1.hl.TZ2.31: What are the major products of electrolysing concentrated aqueous potassium iodide, KI(aq)?
• 18M.2.hl.TZ2.3c.v: Deduce the gas formed at the anode (positive electrode) when graphite is used in place of copper.
• 18M.2.hl.TZ2.4b: The change in the free energy for the reaction under standard conditions, ΔGΘ, is −514 kJ at 298...
• 18M.2.hl.TZ2.4c: Calculate the standard electrode potential, in V, for the BrO3−/Br− reduction half‑equation using...
• 18M.1.hl.TZ1.29: What are the products of electrolysis when concentrated calcium bromide solution is electrolysed...