Which of the following statemen f6boeem72e)o)q-c rvts 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 condiki on /qf7ag/4r*e+pdtions for standard cell potentials?ao epq rkd i*n/47f/+g
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is corr0fmc f;v,vs26 qiyw*ject?

  Which row of the table is correct for a sponscg-) 3o na.d,udcwv3taneous reaction?

  Which statement about elect.q58ahjx -i, 5bkzkww7h elw3fe+;f trochemical cells is not correct?

  What are the correct products of the reaction of nitric acid and man. a4hpqk0r1 -n-guu ngnesium metalrn1 q.uagk--n 0hnp 4u?

  Which statements about the electrol0f,35s:ksm, 4o djlt0rczt.3c ur xgmysis of molten aluminium oxide are 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 cc s2p)8pkdqu; dwjxlf41.b9 in the table below, contains the correct species that are produced at each electrode during the electrolysis of molten zinc chloride?cxs ; kw)cppdj. 8lqb4u1 9d2f

  Which solution does not produce oxygen at the anode when electrolyzed with inerter u sjgbp2(5/ e/ 2pejb5(rugs lectrodes?

  Oxygen and water are produca cmsij, os5+.h/k ta1ed when nitric acid reacts with potassium manganate(Vk ao+mstisa ,5h1/cj.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 are kffa8)/ec qlr l*s1 /3-qmeuv 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 voltaic cell. The overall reaction taking place i hr,ekenn r119n the cell i91,eker nh rn1s:
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balanced chemdx 8 yn:s -p,k/oi evo2w7em9pical 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 silver is incorreknue9qxyus i+5sd)qk5ou6k7 ;aa ,-d ct?

  What happens to the , p:r6gw3w6fanif m(p- ohta($Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under rwzdf.c *zn/n+1di06arzhf 8c eflux with an aqueous solution of the oxidizing aa*c.h6z+ fndz 1rn /c fd8iwz0gent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cemhag mv(k;0+byhvo b5ez (i:-ll notation given below and the standard electrode potentials, determine the standard cell potential of thevha5b i-(hzbg +o(kmevym;0: 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 are transfeapf*o6/ +dn+jk-z afdrred in the equation for the oxidation of ethanol in the presence of acidified potassium dichromate when balanced with whole numbero6afj f-pd a*/k+n+dzs?
$Cr_2O_7^{2-}(aq) + 14H^+(aq) +6e^- \rightarrow 2Cr^{3+}(aq) + 7H_2O(I)$
$CH_3CH_2OH(aq) + H_2O(I) \rightarrow CH_3COOH(aq) + 4H^+(aq) + 4e^-$

  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 thp:.(*0iyx if- gvfsw je electrolysis of molten sodium chloride. Label the direction o:vg i* sj.fy(xfiwp0 -f 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 reactions shows the oxidation oeu+8h w9xm9/ o7tnqn4- wt l s:tx5ialf a secondary alcohol?

  The diagram below shohjb z ,8 u8kf/3jjn.nlws a Daniel cell. Zinc is more reactive than copper. When the cell is 8,.hjj8/n bzklj3fn uoperating, which statement about the ions in the cell is correct?

  What is the reducing agent in thi r*wk.j05 uircs 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. At which w9*ip7y ejvr7py e)n4h+ma- melectrode will bromine form, and what is t+-7jve)4 y*9hirwemp7p many he process taking place there?

  The diagram below shows a Daniel cell. Zinc i2 f0o fe*5d3xqojb ph1s more reactive than copper. When the spontaneous reaction occurs, which statement about thbeof32 5pq fj0xhod1* e Daniel cell is correct?

  The equation for the overall reaction in a voltaic cell is:i*y(sy 3oqo rp*r6*r4v umd4n
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$
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 followid leh45fyh k45m l)0ning sulfur-contaikmh4yhl40)d i5 fn5 elning species?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to formyhv9xj-h .q0 z 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 ox .raqy +mg,-changes to nitrite ?

Sodium metal may be obtaineda mna g1:6ja f:fulx 9/ oouf35ery4n3 commercially from the electrolysis of molten sodium chloride in a Downs ce 94n6u j13ruoea fa:/f3lofg :xnam5y ll. 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 hn(b ll jfhr292w/o*dzr1(uab:i gdm;jq9+ l 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 react9e4h8 zve*h hodcu-pd9 q6f 6uion:
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
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 celle6wpn. :x2dpki lw 4,g with a standard 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 described below, iq uw+3 -pn* ft8w2sgtspecify its type and write its complete balanced chemical equation using the structural formulas of reactants and 8upsn *3f+-t2wt wgq iproducts.
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 th(-;rx l 5iad5n ocl y, qy*lp;ss9)bthe percentage of copper present in op;55d)ri; ny(yl la9 t -,lqcbs xsh*a sample 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 involvinsxm2z/ m1c 4s fw/+dmnlk4*1j kqe oh;g metals and their aqueous nitrate solus1 mo zlmhej*4kx/ 4fw sdq;+m/kc1n2tions:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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: r-okot l-mgg:;etr0*r tmm45rm0g 1f
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction betweex:j g6,j h;9 7gq q+p:zsqw4azsyjinqg9i 9d9n concentrated sulfuric acid and potassiu;9s, i7 :gzw4gi+99qqqhngqjj ys6pj:zd x9am iodide.
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 equatio7dfkouh mr9 .bnetob1t6ryt 8ol ;7/.ns:
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