Which of the followingc7: )4mk:0nd yd4nsg lsxo6 un statements are correct?
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 avs-bwtt)b) db3 q 65uore the standard conditions for standard cell potentials?)3)6 sbw 5duo-tvqbb t
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correcarlo1 vr-q3u1 0w,kl at?

  Which row of the table is correct for a spontaneous u t5 53a,fbgna)avhs 7reaction?

  Which statement about electrochemical ci* 0lbfx d-*(fec8ku0ibyx p 7ells is not correct?

  What are the correct products ofck 3p8qrm h:l2 the reaction of nitric acid and magnesium metal?3 kqm c2lr8ph:

  Which statements about the electrolysis of molten aluminium oxide ar(zom h- 7ifxccz(u4,s8wzl (ue correct?
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, contains 8arx+rivc n/s4(8nxa the correct species that are produced at each electrode during the(v xarac 84s+i8x/rnn electrolysis of molten zinc chloride?

  Which solution does not produce oxygen at the anode when electrolyzud6y w:xkt. a0/o d1ia.r znbw5 d)vi7at1uo8 ed with inert e0tdd. drokiwu 8ti /:n7awau.1o a15y 6xvz )blectrodes?

  Oxygen and water are pro6u zu2g7,jqw29vbv wbduced when nitric acid reacts with potassium manganate(Vqvg7uzw,jb962 b2 uvw II),$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 arepc rvaoj8/ j0l.xqq1hvf./j e ye-. i3 correct about an electrolytic 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 shows a voltal1 g cs29oakp.ic cell. The overall reaction taking place in the cell is: kc gs921.lopa
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balanced chemical equatio0.favj(memu -+ ;hf1stps.shn 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 object with eojm/1fs4 eo llnwa/)k4)j3 v silver is incorrect?

  What happens to the kr xt92j drr)we0ng+ 3$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under,m-xm6abqj hga zz2+. reflux with an aqueous solution of the oxidizing m6- hjg x,+qaz.za2 mbagent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notatio/l*uc/3t d.ri6 +daytcunjkk)b d *l9 n given below and the standard electrode potentials, determine the standard cuy9t* /.ckardljib lnd* ut) k+/6d 3cell 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 mole;(fxb,cjcv ; zcz0wl7 3cxv9ns of electrons are transferred in the equation for the oxidation of ethanol in the presence of acidified potassium dichromate when balancewz37x,c;cv jfcl x nv;(zb9c 0d 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 el8 d4c+7xi auxoectrolysis of molten sodium chloride. Label the direction of elect4a+c7ix ouxd8 ron 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 reactions shows the oxidatiovjt qe4vec *l,0 8x*,ti ewbi(n of a secondary alcohol?

  The diagram below shows a Daniel cell. Zinc is more reactive than copperya6p q9p;8+tpv*nhfe . When the cell is operating, which statement about the ions in the cell is ayp8 qnp ;h+f*pte9 v6correct?

  What is the reducing agent -j1rxoie+ 0o:dlwe +uin this reaction?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram shows an electrolytic cell. tv,.gjtv j-akd .cs04kp86 ymAt which electrode will bromine form, and what is t0kd ypg8jkm,t6a. -.jv vst 4che process taking place there?

  The diagram below showsaq0xy: np) 4gwc1s8sr a Daniel cell. Zinc is more reactive than copper. When the spontaneous reaction occurs, which statement about yx 8n1r)gca4qs :0psw the Daniel cell is correct?

  The equation for the overall reaction in a voltaicdjg- lb 3fp2uh1 ,+ysq 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 oxidatw5sg,rm m 53lvion states of sulfur in the following sulfur-containing species? vg 5sm53lw m,r
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react wve :fp8 8hgn:psbll(- ith water to form metal hydroxide and 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 to8+2r d9i,vts xtothjvi8v o.; .x jrb8 nitrite ?

Sodium metal may be obtained cx+xj9g0 tt rp;glso1o v,fj9dr:0+j aommercially from the electrolysis of molten sodium chloride in a Downs cell. This cell operates9vl;jt r fp+jo : x+09g1d,gjrtxa so0 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 orgm qs2,1 5e0p gfnb-pf 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 reactah uos(*g,+-) v xe q/4: vvyvij6rvywion:
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
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 cell potential oengfy s-lkey4v*d2z6uo 42: 38h ohulf 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 described below, w a1k0,mutfy s mus2m;*0hb6z u3q-tg specify its type and write its complete balanced chemical equation using the structural formulas of reactants and 2uttf,1m k;a*gsw6 -03zymq bhums0uproducts.
1.Formation of butane from but-2-ene.
2.Formation of but-2-one from butan-2-ol.

  Titration technique can be used to dete hc)7u)sdu55ev,amr e rmine the percentage of copper present in a sample ahse)v7c5 euu5 dr)m,of copper (I) oxide. The sample is first dissolved 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 metals avg,t 6 t2jdq ecfty66 6y *+w, pnvqlew3,eo*cnd their aqueous nitrate solutions:tjyv 62*+ty6qco6n*,6gv et ,wp3l, cfe wdqe

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 reactions:0sec4qyh 92x q
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction between concet 8of5/ 9vednw2uy 3wrntrated sulfuric acid and potassium ionodr ww/ 52ft8e9u3vydide.
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 equf9/eqcvq cw yz;i,h;. ations:
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