Which of the following stats1s*irj 08mw cements 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 standard1.tebkfe(/ yj breu1 mkum )2g1 -t/bt conditions for standard cell potentials? .j1k/km/e- murft ()gb yteb1 etu21b
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is corr(-63 cgix )akk kdil3yect?

  Which row of the table is cc)t 7s3)tw nk1kfp10sakdd e: orrect for a spontaneous reaction?

  Which statement about ey t o bkm;g1 lx:guet5v9r,/h7lectrochemical cells is not correct?

  What are the correct products of tnaj*o/xmx:my7 f y 5l;imo 7h)he reaction of nitric acid and magnesium metal* /m5aliy7h;fj xxyom:7 mno) ?

  Which statements about thr. i2ayul sh -+ pa-m:3yf*eabe 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 ta3l+rv la91a6y i uybx8ble below, contains the correct species that are produced at each el3l9a b l86 yrxv1yau+iectrode during the electrolysis of molten zinc chloride?

  Which solution does not produce oxygen at the anode when electrolyzed with jhb+r7 dajz-a.un/d isz7e(h1w 6tb3inert eleebh t7/n1-6j.zhs3+jbdza7r wi ( udactrodes?

  Oxygen and water are producex10.b bz ,oxj)ddu 7aed when nitric acid reacts with potassium manganate(VII), xj)u ddb.z 0oa7e1xb,$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 arem04+ 7pj jmxar1b5af4 yhcj279w ctag 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 overal redr8qe54sbja0,x ,kl reaction taking place in the ,rk rs,xae bj 5d048qecell 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 equan,q y/h ayz wbq 1rmi03f,98ybtion 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 electroplagdi( l qoq2 xcjl6w a/)3idr7s2o b45oting an object with silver is incorrect?

  What happens to the lb),at c -p;zxb3ur3a$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heaterpdjqy. ;xliv,lwx )/8b 2e( vd under reflux with an aqueous solution of the oxidizing ag lvqibd e2x (xy,.rpv8l/)jw;ent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notatioyy f3oan.*m*r ny y5g7n given below and the standard electrode potentials, determine the sy3*nr.y mgy fo *57nyatandard 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 are transferr,6 tdvw.cc 9nrmttu7 2ed in the equation for the oxidation of ethanol in the presence of acidified potassium dichromate when balanced with whole numbersdtc. m,cw 6t9ut2 rn7v?
$Cr_2O_7^{2-}(aq) + 14H^+(aq) +6e^- \rightarrow 2Cr^{3+}(aq) + 7H_2O(I)$
$CH_3CH_2OH(aq) + H_2O(I) \rightarrow CH_3COOH(aq) + 4H^+(aq) + 4e^-$

  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 electrolys 5xeblp ;+npdt,kwjeb 0m*nxt7x1vac .k.s 12is of molten sodium chloride. Label the direction of e,; w 07s.x.e5vj+k txtb2nd1ncbe1xklm* app lectron 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 react uvrt0wmxuz3 hj.89 x0e((s;bi n4cl gions shows the oxidation of a secondary alcohol?

  The diagram below shows a D;adw al7qi,ep)4l c t3aniel cell. Zinc is more reactive than copper. When the cell is operating, which statement about the d l47lwt,p)ca i3q;aeions in the cell is correct?

  What is the reducing agent in this reaction?x8gvp74:b2 z n(dwk+4m s ugjuhff 5.t
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram shows an electrolytic cellfggyj5p8g ae ;rd1n-/. At which electrode will bromine form, and what is the prg5y;n-8gf/ r a djpg1eocess taking place there?

  The diagram below shows a Daniel ce ;9i4;rwvr ) h fws,gb 1mkv4(tvlrd6jll. Zinc is more reactive than copper. When the spontaneous reaction occurs, which statement agvjh)4;fiv,s6r9twm;k vdw( 1r4r b lbout the Daniel cell is correct?

  The equation for the overall reaction in a volta dzrcvq;,b/ s.sj+ge 6ic 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 following sulfur-cyr+j8lbt j)uk5m ohs6+ ,hr m.ontaining speciesu y m65+h lkbstmh+j ,).8rroj?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to forgl7ownt71pi .a)n l+z(qp ty*a*. xhsm 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 iwr ;em1g ; +gcb 0i5)hcgxf -c-cvr2swjgp8) to nitrite ?

Sodium metal may be obtained 52xuz afkh47 p cs+wz4commercially from the electrolysis of molten sodium chloride in a Dosuk54 +2pzc faxwh4z7 wns 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 of mo*+on .dzrg lqlo4uknob+74i/ lten $CaBr_{2(l)}$ 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 redoxwn o;4ku;p nk- 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 sta) tcbllxrc6e/;rgx vj+t/+: undard 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 and write its complet93d qxyosw7x z6-*-ohs .kvdi6 fh3cwhfw4z + e balanced chemical equation using the structural w-k.zdxqz6*3h4yw367os i cwv9o + xh-d f shfformulas 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 of copper pryw: n bc9vo1skf.8iz 7esent in a sample of cc1n.zs oyw7 :i8kv 9fbopper (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 invcrhm+lb q+0t3ic2 p h2olving metals and their aqueous nitrate solutions:qh22i3r b p0c+tclhm+

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 reactiqs bzf.7:rt j1 eth.*)bepvf,ons:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction between concentrated sulfuric acid and pot ,xi/3meute, uassium ieim xeu,t,/u3odide.
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 equ*dzlpn+w.q,:re1eq f uip1 b( 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