Which of the following statements kpc3s2dyf;4a blx4 b+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 are the standard conditions for standar,0uc wp vsv/ce57b o)kd cell potentials? su)e05p oc ,wc/k bv7v
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correc 4w0jvrv/xbgztf 48*arr 0sa6t?

  Which row of the tab; eu5q;4/orr x5 pwpf*5 tqtg3v8mdrple is correct for a spontaneous reaction?

  Which statement aboutcm(/pa19)smbyb 4sq0uk0r3 ubu, flv electrochemical cells is not correct?

  What are the correct productsi 6cralqxfb. ,u r(kz*6:q;x c of the reaction of nitric acid and magnesium metal?;* kxz(.urfxc bc:qi66, r lqa

  Which statements about the electrolysis of molten aluminium oxide are correct? n/1avr fa ;*cj
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 the correct spec:g:-r7lbmykk 1jd3rub k tb9 zn4l.6ries that are produced at each ele 4.l:jbk -b7:rr 9blrdk3 n6u1ytmgzkctrode during the electrolysis of molten zinc chloride?

  Which solution does not produce :ykcg2nkm3c yo 7 dvta :;a+ ftk11ih*oxygen at the anode when electrolyzed with inerttdn+3hvygay: *cf7 o2: kak;1m1ictk electrodes?

  Oxygen and water are produce97df j7 uwcj34 f*w d4jomvb2od when nitric acid reacts with potassium manganate(VII),vu 3 o*b9w7mc2w7fjj o44djfd$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 electrolytic ca4f9j ubv8y)qell?
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 voltaic cell.1rxgium.cy*r u8x1z;4 ft /my The overall reaction taking place in theyymiz4cx8 1gu tf ;/* xr1.urm cell is:
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balanced chemic .1:el8ky inpyefkw-: al 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 object with sil7tjsso3xabbxt19o, 9ver is incorrect?

  What happens to the ( s)qvo,vi4 rr$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under reflux with zpwje p c64 4c+) 7j8 *pqgnqqxb**czaan aqueous solution of the oxidizing agent 4)pg*6*zc* z4cq n e j87ba+qppwcqxj$KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notation given below anidoaj 2gnizig:v,l *gcc8)4r 236pped the standard electrode potentials, determine 2ig, 84)oj6*gzl2i ap3incv rep: gd cthe 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 ma xnbs3(nqr29d yg4bo:ny moles of electrons are transferred in the equar dn34:ybnx 9qb gs2o(tion for the oxidation of ethanol in the presence of acidified potassium dichromate when balanced 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 electrolyti(ar5gjh1k 3qr1re1t 7sob *lic cell for the electrolysis of molten sodium chloride. Label the direction of electron flow and theji hgqeo3r ar(t11rlk51 *sb7 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 oxidation of a secondary a)b i y:ctn*u-dlcohol?

  The diagram below shows a Daniel cell. Zinc3xo71hxc(31 1nzcxs ;oa guy t is more reactive than copper. When the cell is opoz71x;1tyxa gx c3h(1on 3 cuserating, which statement about the ions in the cell is correct?

  What is the reducing agent i33dgg,jo t1i m(xxyx.h3jbjp 9prn 99n this reaction?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram shows an electro;tr0u)ge: qj ylytic cell. At which electrode will bromine form, 0yur)jqgte: ;and what is the process taking place there?

  The diagram below shows a Daniel cell. Zinc isuulc6c 5 ejk,8 more reactive than copper. When the spontaneous reaction occurs, which statement 5kc u,uc8j6el about the Daniel cell is correct?

  The equation for the overall re+zndd wr6- 2(qaiky-uaction 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 inh;h a qqdk (a*e1oo6i4 the following sulfur-containieiqh 4aoo;(1aqhk6* dng species?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to form metal hydroxide anu. ph:. q3v.pdg/dnwxm bzg b oi/b.hhy))v8;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 changesub*ql s jus(w)s1;xx;)u+qx .y kad( v to nitrite ?

Sodium metal may be obtained commercially from the electrolysis o;4;cn(jtp ux :gxl.2vkz yo ,xfth)(ygb:m/ lf molten sodium chloride in a Do j4not (,l2gf:xhbkp/um;yczlgy. :;x() xvtwns cell. 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 cu lm19jpa6xer: r- 7wof 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 reac swb-rjh0 o);bj.gn g6tion:
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
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 poawh+j:27 cutetential 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 described dbrs-*xap/k2 u7pn/sx 8mf +ybelow, specify its type and write its complete balanced chemical equation using the structural formulas of reactants and products. / kbxux+n rpf* sda m-782spy/
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 percentage of coxv0mt7 gyi3 ry-qk1 9k su:s1tpper present in a sample o7ks9t0 kri- 3s1vty:mgq1u xyf 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 invyq zgb2mlsv.r*viy/lc::+0 q x8 z+ lbw1 can/olving metals and their aqueous nitrate soluti:g+z.8l b/12c nbv*sm xyrzq/cwl +:iyv0al qons:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 followi,l4 h lfv7j3tnng reactions:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reactc3obfasc p7a(0 dkg2 5wsm 4j2ion between concentrated sulfuric acid and potassium iodm c0ag25cs( f4sw2boa3dp7 jkide.
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 equata)x geg0o*9 fs ;abg2qions:
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