Which of the following statements are correcb)c27h qltr8.* ;)zrkhjn,ttr ,fo be t?
I.Voltaic cells convert chemical energy into electrical energy
II.Electrolytic cells convert electrical energy into chemical energy
III.Electrolytic cells require a salt bridge

  Which of the following are the standard conditions for standard ceshc 8jwb gz8 .yv/j5c4ll potentials?v4/.wzy 8 bj8c sgjhc5
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is corre(tmd nj) (dy*t ku0or1ct?

  Which row of the table is correct for a )whzct86 yqw a *.n9:cva(z gmspontaneous reaction?

  Which statement about electrochemical cells g6 4pmgi- ,wj),i wm(gj ,bmqfis not correct?

  What are the correct products of the reaction of kz3 o /pt8lg-hnitric acid and magnesium metal?-/h8opz gtk3l

  Which statements about the electrolysis of molten aluminium oxide are correct? (k-rmlnb 1:u s
I. Aluminium ions gain electrons at the cathode
II. Oxide ions lose electrons at the cathode
III. The cathode is the site of reduction in this cell

  Which row, indicated in the table below, copvm95xj,4jj y p h6ls, +wi.-lw/dpwjntains the correct species that are produced at each electrode during the electrolysis of molten zinc c w sj lwpphl,ivw,j9-j. x4pj+ym /6d5hloride?

  Which solution does not produce oxygen at the anode when electrolyzed with ini0esix*q)ig 9u:8oh kert electr :gs9i0xe* k o8ihqiu)odes?

  Oxygen and water are produced whekf1zh2rx.xuokh . 1q0n nitric acid reacts with potassium manganate(VII),ko2zu 1xx h1.r 0fkhq.$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
1.Define reduction in terms of electron transfer.
2.State the oxidation state of manganese in $KMnO_4$ and in $Mn(NO_3)_2$.In $KMnO_4$:X= ----待选择----+-   , In $Mn(NO_3)_2$:X= ----待选择----+-   
3.Identify which species has been oxidized in this reaction and specify the change in oxidation state it has undergone.

  Which statements are correct about an electrolyt. 2qy xsjd*faqh6 6w hsb1r;w6ic cell?
I. An external power supply is used to drive a non-spontaneous process
II.Oxidation occurs at the positive electrode in the cell
III.The cell could be used to extract a reactive metal from its molten salt

  The diagram below showsge cmxa *(8i hi*.s0xd a voltaic cell. The overall reaction taking place in the cs.ig *x8hxdia(m* e 0cell is:
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balancedg z1625cqk lb/*wvqvy chemical equation and $E^{\theta}$ cell for the spontaneous reaction between the following half-cells?
$Pb^{2+}(aq) + 2e^- \rightarrow Pb(s)$ -0.13V
$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ +0.34V

  Which statement about electroplating an objeqv.51azxxr kz,kguo zrd6) 57sq/ie: ct with silver is incorrect?

  What happens to the vk2sf meic7ed t//pm )/-hgne28l 9wg$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under reflux with an aqueous solution of the oxidizi 2mfnb4l dcj b+c;8pj)mp. g91k8ogkhngnmg mc198b4jc .8jpg;op+l2 )kkhfd b agent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notai5 i6b/nwvqhn 2fl1(a tion given below and the standard electrode potentials, determin2a5(i1 ibf6qn lnhvw/e the standard cell potential of the cell,$E^{\Theta}$.
$Pb(s) | Pb^{2+}(aq) || Ag^+(aq) | Ag(s)$
$Ag^+(aq) + e^- \rightarrow Ag(s)$ +0.80V
$Pb^{2+}(aq) 2e^- \rightarrow Pb(s)$ -0.13V

  Using the following half reactions, how many moles of electrons aqzpt s(z7h uwypn ,h 4dw6-;5zre transferred in the equation for the oxidation of ethanol in the presence of acidified potassium dichromate when balanced-ht5,zq( w7zzpp4su dynw;6h with whole numbers?
$Cr_2O_7^{2-}(aq) + 14H^+(aq) +6e^- \rightarrow 2Cr^{3+}(aq) + 7H_2O(I)$
$CH_3CH_2OH(aq) + H_2O(I) \rightarrow CH_3COOH(aq) + 4H^+(aq) + 4e^-$

  Electrolysis of $Cu^{2+}$ using a current of 1A for 10s produces x mol of Cu metal.
If Q= It, how many moles of Cu metal is produced if $Cu^+$ is electrolyzed under the same conditions?

1.Draw an electrolytic cell for the electrolysis of molten sodium chlor.i m6. oni2/g7o,+y8 -f)gh(uajrexrq eqw c jide. Labe)cgqjj7r x+- h/ieoq,.naw(fu2 .i r o6g 8eyml the direction of electron flow and the polarity of the electrodes.
2. 1.Deduce the major products if dilute aqueous sodium chloride was electrolysed instead.
2.Deduce the major products if concentrated aqueous sodium chloride was electrolysed instead.

  Which of the below rea92bqn h y ,xn. asq7a;ao;3pchc ej.+dctions shows the oxidation of a secondary alcohol?

  The diagram below shows a Daniel cell. Zinc2k 8/.egu d ju-ey0il6r2 ,a 7vbrsjod is more reactive than copper. When the cy6 jea,o /r-jd.vkb0gs d822iu7 re ulell is operating, which statement about the ions in the cell is correct?

  What is the reducing agent in this reactionbk :k)p3te)7v 8gz iyyy *r6dg?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram showsn m)rya1vdzs8hn i3( r23; bw8w7mcys an electrolytic cell. At which electrode will bromine form, and wrsw3h28c sb 1z8 myvnwra i;7md(y3 )nhat is the process taking place there?

  The diagram below shows a Daniel cell. Zinc is more reactive than copper.kp*k 4.oe p 2kqm;yh8v When the spontaneous reaction occurs, which statement about the Da48vp *eokk;y. 2hqmp kniel cell is correct?

  The equation for the overal- x-wj/3mtys k6 m7gell reaction in a voltaic cell is:
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$
Which statements are correct for this cell?
I. Electrons flow from the copper electrode to the silver electrode
II. Silver ions are reduced in the reaction
III. The copper anode will become smaller in size as the reaction proceeds

  What are the respective oxidation states of sulfur in the follow.twi pjihhe(b 3- ,yw4ing sulfur-containyb.jh ,(4i-tew 3pihw ing species?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to form metal hydroxide anc;c; .r(hmsvtf;osmfw o3gzrq k 340 (d hydrogen gas.
1.Write a balanced equation between sodium and water.
2.Explain why this reaction is considered as a redox reaction.
3.3 other alkali metals W, X and Y also react with water.
Based on the following observations, arrange the metals in order, starting from the weakest oxidizing agent. Explain your answer. ----待选择----XYW $\lt$ ----待选择----XYW $\lt$ ----待选择----XYW $\lt$

Meta	Observations
W	Slow reaction with water
X	Vigorous reaction with water
Y	Fast reaction with water

  What happens to nitrogen when nitrate changes to nitrith+k+ sstp f6:6+)iu,r ybbkz ke ?

Sodium metal may be q4ym (jino e0-q-i8xn obtained commercially from the electrolysis of molten sodium chloride in a Downs q-08oiyx(menj4 ni-qcell. This cell operates as an electrolytic cell.
1.Describe, using a diagram, the essential components of this electrolytic cell.
2.Suggest why molten sodium metal may be collected from the top of this type of cell.
3.Describe two ways in which current is conducted in an electrolytic cell.

  A battery is added to a container of th q4yhdkr:3ll(6*2apev4az molten $CaBr_{2(l)}$ to create an electrolytic cell, as shown in the diagram below.



1. 1Use section 24 (Section 19- 2025 Syllabus) of your data booklet to identify and write the oxidation and reduction half-reactions.
2.Label the anode and cathode on the diagram above.
3.On the diagram above, label the electrode where calcium metal $(Ca_{(s)})$will appear.
2.A different electrochemical cell is shown below. One half-cell contains a lead metal electrode immersed in 1.0 M $Pb(NO3)_2$ solution. A standard electrode potential table is also shown for elements X, Y, and Z.

Elements	Electrode potential
$X^{2+}_{(aq)} + 2e^- \rightarrow X_{(s)}$	$E^{\Theta}$=-1.18V
$Y^+_{(aq)} + 1e^- \rightarrow Y_{(s)}$	$E^{\Theta}$=-0.45V
$Z^{2+}_{(aq)} + 2e^- \rightarrow Z_{(s)}$	$E^{\Theta}$=+0.34V

1.Label the left half-cell of the diagram with the metal that will produce the highest cell potential.
2.Draw an arrow on the diagram indicating the direction of the flow of electrons.
3.Consult section 24 (Section 19- 2025 Syllabus) in your data booklet to calculate the standard cell potential for the diagrammed cell.  V
4.Use metals X, Y, and Z combined with aqueous chloride solutions of metals X, Y, and Z, and write a balanced equation for a reaction that will proceed spontaneously.

  Consider the following redox reaction:5;(vn 3 dhy byvlutze/y/mt*8
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
1. 1.Using section 24 (Section 19- 2025 Syllabus) of the data booklet, calculate the standard cell potential.  V
2.Predict, with a reason, whether this reaction is spontaneous or not.
2.Using sections 1 and 2 of the data booklet, calculate the standard Gibbs free energy change in $kJ\,mol^{-1}$.
The standard entropy change for this reaction is $508J\,K^{-1}\,mol^{-1}$
3.Using section 1 of the data booklet, calculate the standard enthalpy change for this reaction in $kJ\,mol^{-1}$.
$\Delta G^{\Theta}$=  $kJ\,mol^{-1}$, $\Delta H^{\Theta}$=  $kJ\,mol^{-1}$

  The Daniell Cell is a galvanic cell with a standard r+jwonv knz:*km3 /n/cell potential of 1.10V.
$Cu^{2+}(aq) + Zn(s) \rightarrow Cu(s) + Zn^{2+}(aq)$
1. 1.Define standard electrode potential.
2.List the features of a standard hydrogen electrode (SHE).
Suppose the SHE is replaced by a MMSE reference electrode with a standard electrode potential of 0.64V.
2. 1.Using section 24 (Section 19- 2025 Syllabus) of the data booklet, calculate the new electrode potentials.Cu(s):  V, Zn(s):  V
2.Using your answers to (b)(i), calculate the new cell potential and comment on this value.$E_{cell}$=  V

For each reaction describe(0 f0q2kuu4jo6fs xbc d below, specify its type and write its complete balanced chemical equation using the structural formulas s4 ff0(2ock qujux0 b6of reactants and products.
1.Formation of butane from but-2-ene.
2.Formation of but-2-one from butan-2-ol.

  Titration technique can be used to determine the per. -k3 di;-a mmgm2p.ylh;ktrh centage of copper present in a sample of copper (I) oxide. The sample is first dis; -3; m.laim2k-y hr.kpg tdhmsolved in acidic solution and $Cu^+$ ions are formed. The resulting solution is then titrated against a standard solution of potassium manganate (VII),$KMnO_{4}$. In acidic solution,$MnO^-_4$ reacts with $Cu^+$ to form $Mn^{2+}$ and $Cu^{2+}$ ions.

Titre	1	2	3
Initial burette reading/$cm^3$	2.00	24.70	5.00
Final burette reading/$cm^3$	25.80	48.30	30.60

Mass of copper oxide (I) sample/g 0.7751
Concentration of $KMnO_{4}$ solution/$mol\,dm^{-3}$ $2.375\times10^{-2}$
1.Using Section 24 (Section 19- 2025 Syllabus)of the Data Booklet, write the equation of the redox reaction.
2.Define reducing agent and specify the reducing agent in the reaction.
3.Calculate the number of moles of $MnO^-_4$ that reacted with $Cu^+$.  $cm^3$
4.Deduce the percentage by mass of Cu present in the sample.  %
Important note: The section numbers mentioned in the video solution are specific to the 2024 syllabus.
You can refer to the question stem to find the section numbers in the 2025 syllabus.

  Consider the following reactions involving meta2 rnaj (iuvrke9 gvdb(b(8d96 ls and their aqueous nitrate soluti j86i bu9g(nerravb9 vd(dk2(ons:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
Metal X		No reaction	No reaction
Metal Y	Grey solid of metal X observed		No reaction
Metal Z	Grey solid of metal X observed	Pink solid of metal Y observed

Choose the correct order of the metals from the strongest oxidizing agent to the weakest?

  Consider the following re:4vr n9t, kuteactions:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction between concentrated ssgjm.)2iwt3 wulfuric acid and potassium ij.wm 3iwgt s2)odide.
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
1.State the oxidation state of sulfur in $H_2SO_4$ and $4H_2S$.In $H_2SO_4$, x= ----待选择----+-   , in $4H_2S$, x= ----待选择----+-   
2.Write the half equations for the oxidation and reduction reactions.
3.Define oxidizing agent in terms of electrons.
4.Identify the oxidizing agent in the equation.

  Consider the following equations: ogdzyq-.ml6v52 w5ogjbr r(g.jk7u 3
Equation 1:
$2ClO_3^-(aq) + I_2(aq) \rightarrow Cl_2(aq) + 2IO_3^-(aq)$
Equation 2:
$ Cl_2(aq) + 2NaOH(aq) \rightarrow NaCl(aq) + NaClO(aq) + H_2O(l)$
Which statements about these reactions is/are not correct?
I.Iodine is reduced in equation 1
II.Chlorine is reduced only in equation 1
III.Chlorine is oxidized and reduced in equation 2