Which of the following statements are correcgodtkv ry7pz:o ,w xf*0fp 95k 7qt*y+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 thlveinfunmn 973-.e ff 8e-dh(e standard conditions for standard cell potentials?l38h( eu - fv.f9- ne7neidmnf
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correct?-kt u v(lsdey;b *e66o

  Which row of the table is cogewz/q(lz4 (. 5eznza rrect for a spontaneous reaction?

  Which statement about electrochemical cefz6.li ;ld)9u*y ust hlls is not correct?

  What are the correct products of the reaction of nitric acid adw t8 iyqw:+hr9zzk/+nd magnesium metal?wk zdt:z+9wi /8h+rqy

  Which statements about thaq ilpe(j g1j0n /tu)*4i5bgd e electrolysis 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 in the table below1r8uszq8e + np, contains the correct species that are produced at each electro 8 nrpzu8+sqe1de during the electrolysis of molten zinc chloride?

  Which solution does not produce oxygen at the anode when electrolyzed c2gvqhf2i16* +q 5p svsc6v cswith inert electrodesv*sq5 6+2c1vh pc qfcgi26svs?

  Oxygen and water are produced when j,b(foa 9ri6jiv+7pb nitric acid reacts with potassium manganate(VIIa j(v9p 6 ij,frbo+bi7),$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 a 93ie ct 8q g5 y.wbxa1gcfpxe7y4tt59bout 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 t+y j kd:sjvn7: vrbv/y xr3:(overall reaction taking place in the cek ybd:jvny7 +:x(v rsv/3: rtjll 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 chemical equatioo0e yd9;xp+zn n 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 wit /f)m;ndd./gz:gru/k md t l*lh silver is incorrect?

  What happens to the db2bws zk- : znfj:mq6jxi.:, $Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under zbsfuvsa5 ,28/x mbd6 reflux with an aqueous solution of the oxidizing agenabm6 u,zdfs/ vbx2s5 8t $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notation given below and thxc7+ ;y1 wec af6sq*ohe standard electrode potentials, determine the standard cell potentwf eyx *o;+s1qh7c6a cial 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 are transfef( v62e.-j,l ux pvd kinx;l+brred in the equation for the oxidation of ethanol in the presence of acidified potassium dix- vf .(in ej+,vlx;du2lk p6bchromate 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 electrolytic cell for the electrolx m0s+7a-ur.m 3f cplrysis of molten sodium chloride. Label the direction of electron flow andapfsc.+r l x03ru-m 7m 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 s)m zmrw.*88inb buq)fhows the oxidation of a secondary alcohol?

  The diagram below shows a ry,taok1 u6 k0 m:r5tkDaniel cell. Zinc is more reactive than copper. When the cell is operating, which statement about the ions in the cell is corre, ykttr:ao1 ukr0k65mct?

  What is the reducing agent in th qqsy rf-a).lh8+qub; w1o*2)j bdafjyb :c1j is reaction?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram showoxgd* yo h450as an electrolytic cell. At which electrode will bromine form, and what is the process taking place there0o dy4oxhg *a5?

  The diagram below shows a Dani3f,m ubbu + )x;tnj4vwnlx:-iel cell. Zinc is more reactive than copper. When the spontaneous reaction occurs, which statement:jv;mbuf 3ux t4nw-)+ ,xnbli about the Daniel cell is correct?

  The equation for the overall reaction in a voltaic c -ye zz6acst,5qrwn01( 9qunoell 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 respectiveje7,-ix . vih (9jxmc+e kow3l oxidation states of sulfur in the following sulfur-containing e(x. iki+lej3o,wx- 9vmc h7jspecies?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to form metal hydroxidcov-4 5h2g f -h zeijk:fjxv(/e 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 to nitrie 7m 1h2,c61 z pjl8;bbxmfkso;bss:p te ?

Sodium metal may be obv9*r z/ vjyh *mlu)ip/fp+ df7b qh.j;tained commercially from the electrolysis of molten sodium chloride in a )/i vuyrz;h *pjvfp.fmb+9ql /d*j7hDowns 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 containp6a oevq0:f;t+ mp/n,e ;jp/hev,okr +xnbg9 er of 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 fn.doz.luy ;qcv5)ero q k* i785e zt/reaction:
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
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 lt ftvnd(3j(hb1s9v :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, specify its type and77 jnk6erne3tq p1w 4ny6mv 3lg*gf,h write its complete balanced chemical equation usm6lh 63vf ,gp7ekjtn 4*q71 w3yernn ging the structural formulas of 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 percentage (zd2e-tbu20dsgl*ewag w /; ai14pyvof copper present in a sample of copper (I) oxide. Thedz; ay1s( * aegp/w - dul2bwe2vi4g0t 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 inu 2.r.ugcj yhjb70dv; volving metals and their aqueous nitrate solutions:j.7 juy rg;bu dc2vh.0

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 following44+vrn xp+g;dn q*irs 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 reaction between concentrated wy t,.8rc gy6zvud2*zsulfuric acid and potassiumg6* yt8,u2ywd zrc vz. 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 equfge2byyfm8t 9hv 44 v3nr:m ,tations:
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